Please answer these questions on your Page 7 (a) We place 88.8 g of a metal at 10.00°C in 444.4 g of water at 70.00°C. The water is in a beaker that is also at 70.00°C. The specific heat capacity of water is 4.184 J K-¹ g¹ and that of the metal is 0.555 J K-¹g-¹. The heat capacity of the beaker is 0.777 kJ K-¹. What is the final temperature of the metal, the water, and the beaker? (b) Calculate the enthalpy change for the reaction C(graphite) + 2 H₂(g) → CH₂(g) with the help of the enthalpy changes of the following reactions: C(graphite) + O₂(g) → CO2(g) AH-393.5 kJmol-1 H₂(g) + O2(g) → H₂O(1) AH-285.8 kJmol-1 CH₁ (g) + 2 O₂(g) → CO₂(g) + 2 H₂O(1) AH-890.4 kJmol-¹ The temperature is 25°C in all instances.

3. A 74.5 g piece of metal at 86.0°C is placed in 133 g of water at 21.0°C contained in a calorimeter. The metal and water come to the same temperature at 24.2°C. How much heat (in J) did the metal give up to the water? (Assume the specific heat of water is 4.18 J/g·°C across the temperature range.)  J What is the specific heat (in J/g·°C) of the metal?  J/g·°C 4. A 0.528 g sample of KCl is added to 51.7 g of water in a calorimeter. If the temperature decreases by 1.07°C, what is the approximate amount of heat (in J) involved in the dissolution of the KCl, assuming the heat capacity of the resulting solution is 4.18 J/g°C?  J Is the reaction exothermic or endothermic? exothermicendothermic  5. When 2.56 g of methane burns in oxygen, 128 kJ of heat is produced. What is the enthalpy of combustion (in kJ) per mole of methane under these conditions?  kJ/mol methane 6. Joseph Priestly prepared oxygen in 1774 by heating red mercury(II) oxide with sunlight focused through a lens. How much…

If 30.5 g of LiBr are dissolved 350.0 g of water at 20.0 °C in an insulated container, a temperature change is observed. The Δ H of solution of LiBr is -48.8 kJ/mol. Assuming that the specific heat of the solution is 4.184 J/(g C) and that no heat is gained or lost by the container, what will be the final temperature of the solution?

The specific heat capacity of silver is 0.2386 J/g °C. Assuming no loss of heat to the surroundings or to the calorimeter, determine the final temperature when 100.0 g of silver at 40.0°C is immersed in 60.0 g of water at 10.0°C.

A gas expands and does work on the surroundings equal to 4.92 Latm. At the same time, it releases 98.6 J of heat to the surroundings. What is the change in energy in J of the gas? (write the solution without decimals)

when 50.0 mL of 0.200 M NaOH is mixed with 50 mL of 0.200 M HCl in a coffee cup calorimeter, the temperature increases from 23.5 degrees C to 26.5 degrees C. Assuming that the density of the resulting solution is 1.00 g/mL and the specific heat capacity of the solution is 4.18 J/g degrees C, what is qrxn?

A 37.7 g. piece of an unknown metal is heated up 43.5 °C when given 1,095.4 J of heat.  What is the specific heat capacity of the metal?

When a 6.50 g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter, the temperature of the water rises from 21.6 to 37.8oC. Was the chemical reaction (dissolving the solid) endothermic or exothermic? How do you know? Write a balanced chemical equation for this process. Determine how many joules of heat (q) were involved in changing the temperature of the water. If the heat that changed the temperature of the water was a result of the chemical reaction, determine the ΔH of the chemical reaction in kJ/mol of sodium hydroxide.

A chemist carefully measures the amount of heat needed to raise the temperature of a 639.0 g sample of C,H,N from -8.7 °C to 6.7 °C. The experiment shows that 2.60 × 10* J of heat are needed. What can the chemist report for the molar heat capacity of C,H,N? Round your answer to 3 significant digits. - 1 ·K J• mol х10