Question 1

What is the value of 783 K in units of °C?

Accepted Answer

To convert from Kelvin (K) to Celsius (°C), simply subtract 273. Therefore, 783 K - 273 = 510 °C. Choice C is the only option that matches this value.

Question 2

What is the final temperature of 25.0 grams of water at 22.0°C after it absorbs 454 J of heat?

Accepted Answer

First, we need to use the equation: q = mCΔT, where q is the heat absorbed, m is the mass of water, C is the specific heat capacity of water, and ΔT is the change in temperature. We can rearrange the equation to solve for ΔT: ΔT = q / (mC). Plugging in the given values, we get: ΔT = 454 J / ((25.0 g)(4.18 J/g°C)) = 4.29°C. Therefore, the final temperature is 22.0°C + 4.29°C = 26.3°C, which corresponds to choice C.

Question 3

How much heat (kJ)is absorbed by 948.0 g of water in order for the temperature to increase from
25.00°C to 32.50°C?

Accepted Answer

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Question 4

Given the table of specific heat values below,what is the identity of a 26.2 g metal sample that increases by 8.5°C when 100.0 J of energy is absorbed?
Element Specific Heat(J/g°C)
Au 0.128
Ag 0.235
Cu 0.385
Fe 0.449
Al 0.903

Accepted Answer

The specific heat of the metal sample can be calculated as:Specific heat = Energy absorbed / (Mass * Change in temperature)Specific heat = 100.0 J / (26.2 g * 8.5°C)Specific heat = 0.449 J/g°CThis value matches the specific heat of iron (Fe), which is 0.449 J/g°C. Therefore, the identity of the metal sample is Fe.

Question 5

What is the value of 27°C on the Fahrenheit scale?

Accepted Answer

To convert Celsius to Fahrenheit, we use the formula F = (C x 1.8) + 32. Plugging in 27 for C, we get F = (27 x 1.8) + 32 = 80.6. Rounded to the nearest whole number, the answer is 73 (choice A).

Question 6

What is the value of -25°C on the Kelvin scale?

Accepted Answer

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Question 7

How many joules are in 55.2 calories?

Accepted Answer

The answer of How many joules are in 55.2 calories?
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Question 8

Given the table of specific heat values below,what is the identity of a 10.0 g metal sample that increases by 14.0°C when 62.9 J of energy is absorbed?
Element Specific Heat(J/g°C)
Au 0.128
Ag 0.235
Cu 0.385
Fe 0.449
Al 0.903

Accepted Answer

The specific heat of the metal sample can be calculated as:Specific heat = Energy absorbed / (Mass * Change in temperature)= 62.9 J / (10.0 g * 14.0°C)= 0.449 J/g°CThis value matches the specific heat of iron (Fe), which is 0.449 J/g°C. Therefore, the identity of the metal sample is Fe.

Question 9

How many Calories are in 575.0 calories?

Accepted Answer

The answer of How many Calories are in 575.0 calories?
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Question 10

How many grams of water when supplied with 348 J of heat will gain a temperature of 5.2°C?

Accepted Answer

The specific heat of water is 4.184 J/g°C. So, the mass of water that will gain a temperature of 5.2°C when supplied with 348 J of heat is:mass = heat / (specific heat * temperature change)mass = 348 J / (4.184 J/g°C * 5.2°C)mass = 16.0 g

Quiz 3: Matter and Energy