Question

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A sample of tin goes through a temperature change of -160.56 °C while releasing 36298 joules of heat. The specific heat capacity of tin is 0.227 J/(g.°C). What is the mass of this sample?

A 13.66 mol sample of ammonia absorbs 33834 joules of heat. The specific heat capacity of ammonia is 80.08 J/(mol. °C). By how much did the temperature of this sample change, in degrees Celsius?

A sample of cobalt undergoes a temperature change of -1132.52 °C while releasing 455500 joules of heat. The specific heat capacity of cobalt is 0.4187 J/(g.°C). What is the mass of this sample?

A 372.4 g sample of indium goes through a temperature change of +140.73 K while absorbing
12505 joules of heat. What is the specific heat capacity of indium?

A 4.721 mol sample of molybdenum absorbs 35961 joules of heat. The specific heat capacity of molybdenum is 24.06 J/(mol-°C). By how much did the temperature of this sample change, in degrees Celsius?

A 56.2 g sample of ethanol is subjected to a temperature change of -110.56 K. The specific heat capacity of ethanol is 2.44 J/(g K). How many joules of heat were transferred by the sample?

A 5.774 mol sample of chromium absorbs 38674 joules of heat. The specific heat capacity of chromium is 23.35 J/(mol °C). By how much did the temperature of this sample change, in degrees Celsius?

A 4.9 mol sample of magnesium is subjected to a temperature change of -683.83 K. The specific heat capacity of magnesium is 24.9 J/(mol K). How many joules of heat were transferred by the sample?

A 0.2687 mol sample of tin is subjected to a temperature change of +222.48 K. The specific heat capacity of tin is 27.112 J/(mol K). How many joules of heat were transferred by the sample?

A 1.008 mol sample of neon undergoes a temperature change of -703.43 K while releasing
14738 joules of heat. What is the specific heat capacity of neon?

Answer 1

To solve these problems, we can use the formula:

q = mcΔT

where q is the heat transferred, m is the mass of the substance, c is the specific heat capacity of the substance, and ΔT is the temperature change.

The mass of the sample of tin can be calculated as:

q = mcΔT

36298 J = m × 0.227 J/(g.°C) × (-160.56 °C)

m = 708.2 g

The temperature change of the sample of ammonia can be calculated as:

q = mcΔT

33834 J = 13.66 mol × 80.08 J/(mol.°C) × ΔT

ΔT = 31.7 °C

The mass of the sample of cobalt can be calculated as:

q = mcΔT

455500 J = m × 0.4187 J/(g.°C) × (-1132.52 °C)

m = 27.4 g

The specific heat capacity of indium can be calculated as:

q = mcΔT

12505 J = 372.4 g × c × 140.73 K

c = 0.238 J/(g.°C)

The temperature change of the sample of molybdenum can be calculated as:

q = mcΔT

35961 J = 4.721 mol × 24.06 J/(mol.°C) × ΔT

ΔT = 31.9 °C

The heat transferred by the sample of ethanol can be calculated as:

q = mcΔT

q = 56.2 g × 2.44 J/(g K) × (-110.56 K)

q = -15,585 J

The temperature change of the sample of chromium can be calculated as:

q = mcΔT

38674 J = 5.774 mol × 23.35 J/(mol.°C) × ΔT

ΔT = 27.4 °C

The heat transferred by the sample of magnesium can be calculated as:

q = mcΔT

q = 1.008 mol × 24.9 J/(mol K) × (-683.83 K)

q = -17,134 J

The heat transferred by the sample of tin can be calculated as:

q = mcΔT

q = 0.2687 mol × 27.112 J/(mol K) × 222.48 K

q = 1676.7 J

The specific heat capacity of neon can be calculated as:

q = mcΔT

14738 J = 1.008 mol × c × (-703.43 K)

c = 36.8 J/(mol.°C)

Step-by-step explanation: