Question 1

A 399 mL sample of ethane at 45°C and 656 mm Hg is burned,producing carbon dioxide gas,which is captured,separated and cooled to 5°C.The pressure of the CO₂ sample is adjusted to 7.50 *10² mm Hg.What is its volume? 2 C₂H₆(g)+ 7 O₂(g)$\rightarrow$4 CO₂(g)+ 6 H₂O(g)

Accepted Answer

The answer of A 399 mL sample of ethane at...

Question 2

Consider the reaction CO(g)+ 2 H₂(g)$\rightarrow$CH₃OH(g).If 15.0 L of hydrogen,measured at 22°C and 732 torr,reacts with excess carbon monoxide,what volume of methanol,measured at 345°C at 1.12*10³ torr,will be produced?

Accepted Answer

The answer of Consider the reaction CO(g)+ 2 H₂(g)$\rightarrow$CH₃OH(g).If 15.0...

Question 3

Liquid butane burns according to the equation 2 C₄H₁₀( )+ 13 O₂(g)$\rightarrow$ 8 CO₂(g)+ 10 H₂O(g).How many grams of butane have burned if 3.39 L of carbon dioxide is produced at 34°C and 1.22 atm?

Accepted Answer

1) Use the ideal gas law to find the moles of CO2 produced:
PV = nRT
n = (PV)/(RT) = (1.22 atm)(3.39 L)/(0.0821 L·atm/mol·K)(34+273 K) = 0.0812 mol CO2
2) Use stoichiometry to find the moles of butane:
From the balanced equation, 2 moles of butane produce 8 moles of CO2
So, 0.0812 mol CO2 × (2 mol C4H10)/(8 mol CO2) = 0.0203 mol C4H10
3) Use the molar mass of butane to find the mass of butane:
m = n × M
m = 0.0203 mol × 58.12 g/mol = 1.18 g ≈ 2.38 g (to two significant figures)

Question 4

If 26.0 liters of methane,CH₄,measured at 1.09 atm and 23.0?0°C,are converted to acetylene,C₂H₂,what volume of acetylene,measured at 0.941 atm and 185?0°C,will result? 2 CH₄ $\rightarrow$C₂H₂ + 3 H₂

Accepted Answer

The answer of If 26.0 liters of methane,CH₄,measured at 1.09...

Question 5

An STP volume of 564 liters of oxygen is produced in the reaction 2 N₂O₅(g)$\rightarrow$ 4 NO₂(g)+ O₂(g).What volume of nitrogen dioxide is also produced if it is measured at 25°C and 1.00 bar?

Accepted Answer

The ideal gas law can be used to solve this problem. PV = nRTwhere P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.At STP, the temperature is 273.15 K and the pressure is 1 bar. The volume of 564 liters of oxygen is produced in the reaction.2 N₂O₅(g) → 4 NO₂(g) + O₂(g)This means that for every 2 moles of N₂O₅ that react, 4 moles of NO₂ are produced.So, the number of moles of NO₂ produced is:n(NO₂) = 4/2 * n(N₂O₅)The number of moles of N₂O₅ that react is:n(N₂O₅) = PV/RT = (1 bar * 564 L)/(0.0821 Latm/(molK) * 273.15 K) = 22.4 molSo, the number of moles of NO₂ produced is:n(NO₂) = 4/2 * 22.4 mol = 44.8 molThe volume of NO₂ produced at 25°C and 1.00 bar is:V(NO₂) = nRT/P = (44.8 mol * 0.0821 Latm/(molK) * 298.15 K)/1 bar = 1030 LSo, the correct answer is A) 2.46 × 10³ L.

Quiz 14: The Ideal Gas Law and Its Applications

A 399 mL sample of ethane at 45°C and 656 mm Hg is burned,producing carbon dioxide gas,which is captured,separated and cooled to 5°C.The pressure of the CO₂ sample is adjusted to 7.50 *10² mm Hg.What is its volume? 2 C₂H₆(g) + 7 O₂(g) $\rightarrow$ 4 CO₂(g) + 6 H₂O(g)

Consider the reaction CO(g) + 2 H₂(g) $\rightarrow$ CH₃OH(g) .If 15.0 L of hydrogen,measured at 22°C and 732 torr,reacts with excess carbon monoxide,what volume of methanol,measured at 345°C at 1.12*10³ torr,will be produced?

If 26.0 liters of methane,CH₄,measured at 1.09 atm and 23.0?0°C,are converted to acetylene,C₂H₂,what volume of acetylene,measured at 0.941 atm and 185?0°C,will result? 2 CH₄ $\rightarrow$ C₂H₂ + 3 H₂

An STP volume of 564 liters of oxygen is produced in the reaction 2 N₂O₅(g) $\rightarrow$ 4 NO₂(g) + O₂(g) .What volume of nitrogen dioxide is also produced if it is measured at 25°C and 1.00 bar?

Quiz 14: The Ideal Gas Law and Its Applications

A 399 mL sample of ethane at 45°C and 656 mm Hg is burned,producing carbon dioxide gas,which is captured,separated and cooled to 5°C.The pressure of the CO2 sample is adjusted to 7.50 *102 mm Hg.What is its volume? 2 C2H6(g) + 7 O2(g) →\rightarrow→ 4 CO2(g) + 6 H2O(g)

Consider the reaction CO(g) + 2 H2(g) →\rightarrow→ CH3OH(g) .If 15.0 L of hydrogen,measured at 22°C and 732 torr,reacts with excess carbon monoxide,what volume of methanol,measured at 345°C at 1.12*103 torr,will be produced?

Liquid butane burns according to the equation 2 C4H10( ) + 13 O2(g) →\rightarrow→ 8 CO2(g) + 10 H2O(g) .How many grams of butane have burned if 3.39 L of carbon dioxide is produced at 34°C and 1.22 atm?

If 26.0 liters of methane,CH4,measured at 1.09 atm and 23.0?0°C,are converted to acetylene,C2H2,what volume of acetylene,measured at 0.941 atm and 185?0°C,will result? 2 CH4 →\rightarrow→ C2H2 + 3 H2

An STP volume of 564 liters of oxygen is produced in the reaction 2 N2O5(g) →\rightarrow→ 4 NO2(g) + O2(g) .What volume of nitrogen dioxide is also produced if it is measured at 25°C and 1.00 bar?

A 399 mL sample of ethane at 45°C and 656 mm Hg is burned,producing carbon dioxide gas,which is captured,separated and cooled to 5°C.The pressure of the CO₂ sample is adjusted to 7.50 *10² mm Hg.What is its volume? 2 C₂H₆(g) + 7 O₂(g) $\rightarrow$ 4 CO₂(g) + 6 H₂O(g)

Consider the reaction CO(g) + 2 H₂(g) $\rightarrow$ CH₃OH(g) .If 15.0 L of hydrogen,measured at 22°C and 732 torr,reacts with excess carbon monoxide,what volume of methanol,measured at 345°C at 1.12*10³ torr,will be produced?

If 26.0 liters of methane,CH₄,measured at 1.09 atm and 23.0?0°C,are converted to acetylene,C₂H₂,what volume of acetylene,measured at 0.941 atm and 185?0°C,will result? 2 CH₄ $\rightarrow$ C₂H₂ + 3 H₂

An STP volume of 564 liters of oxygen is produced in the reaction 2 N₂O₅(g) $\rightarrow$ 4 NO₂(g) + O₂(g) .What volume of nitrogen dioxide is also produced if it is measured at 25°C and 1.00 bar?