Energy, Heat, Temperature
The lowest recorded temperature in Canada was −63 °C in Snag, Yukon on February 3, 1947. Convert this temperature to Fahrenheit.
-81 F
Calculate the heat required to raise the temperature of 75.1 g of mercury from 31.7 °C to 53.8 °C. The specific heat capacity of mercury is 0.14 J/(g∙ °C).
.129J/g*C
Calculate the specific heat capacity for a 15.3-g sample of gold that absorbs 87.2 J when its temperature increases from 35.0 °C to 79.2 °C.
.129J/g*C
Calculate the specific heat capacity for a 22.7-g sample of lead that absorbs 237 J when its temperature increases from 29.8 °C to 95.6 °C.
.159J/g*C
Calculate the specific heat capacity for a 13.7-g sample of nickel that absorbs 361 J when its temperature increases from 28.4 °C to 87.8 °C.
.444 J/g*C
Calculate the specific heat capacity for a 32.3-g sample of titanium that absorbs 392 J when its temperature increases from 42.1 °C to 65.3 °C.
.523J/g*C
Calculate the heat required to raise the temperature of 28.6 g of sodium from 33.7 °C to 73.8 °C. The specific heat capacity of sodium is 1.23 J/(g∙ °C).
1.41x10^3 j
Calculate the heat required to raise the temperature of 13.5 g of ethanol from 25.8 °C to 85.6 °C.
1.95x10^3 J
Two units of measurement for energy are calories and joules. The measurement of 25.1 cal is the same amount of energy as ___________.
105 J
The highest recorded temperature in Canada was 45 °C in Midale, Saskatchewan, on July 5, 1937. Convert this temperature to Fahrenheit.
113 F
The highest recorded temperature in Africa was 55 °C in Kebili, Tunisia, on July 7, 1931. Convert this temperature to Fahrenheit.
131 F
Calculate the heat required to raise the temperature of 75.1 g of mercury from 31.7 °C to 53.8 °C. The specific heat capacity of mercury is 0.14 J/(g∙ °C).
2.3*10^2 J
The enthalpy of vaporization of liquid water is 40.65 kJ/mol. Calculate the energy required to vaporize 12.5 g of liquid water.
28.2 kJ
Calculate the heat required to raise the temperature of 52.5 g of gold from 56.3 °C to 98.4 °C.
283 J
The enthalpy of vaporization of liquid isopropyl alcohol is 45 kJ/mol. Calculate the energy required to vaporize 39.5 g of this compound
30. kJ
Two units of measurement for energy are calories and joules. The measurement of 8.75 kcal is the same amount of energy as ___________.
36.6 kJ
The enthalpy of fusion of solid n-butane is 4.66 kJ/mol. Calculate the energy required to melt 58.3 g of solid n-butane
4.66 kJ
The enthalpy of fusion of solid n-butane is 4.66 kJ/mol. Calculate the energy required to melt 58.3 g of solid n-butane.
4.66 kJ
The enthalpy of fusion of solid sodium is 2.60 kJ/mol. Calculate the energy required to melt 43.6 g of solid sodium.
4.94
A 68-g sample of sodium is at an initial temperature of 42 °C. If 1840. joules of heat are applied to the sample, what is the final temperature of the sodium?
64 C
Two units of measurement for energy are calories and joules. The measurement of 32.3 kJ is the same amount of energy as ___________.
7.72 kcal
A 143-g sample of mercury is at an initial temperature of 25 °C. If 1067 joules of heat are applied to the sample, what is the final temperature of the mercury? The specific heat capacity of mercury is 0.14 J/(g∙ °C).
78 C
The enthalpy of fusion of ice is 6.02 kJ/mol. Calculate the energy required to melt 25.9 g of ice.
8.67 kJ
Two units of measurement for energy are calories and joules. The measurement of 355 J is the same amount of energy as ___________.
84.8 cal
An 85-g sample of iron is at an initial temperature of 38 °C. If 2213 joules of heat are applied to the sample, what is the final temperature of the iron?
96 C
A 91-g sample of gold is at an initial temperature of 22 °C. If 874 joules of heat are applied to the sample, what is the final temperature of the gold?
97 C
