A chemist measures the enthalpy change AH during the following reaction: 8 SO2(9) + 16 H,S(g)→ 3 Sg(s) + 16 H,0(1) ДН--1863. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ΔΗ x10 3 280, (2) + 4H,8 (g) → s,6) + 4H,0(1) O kJ 3S,(s) + 16H,0(1) –→ 880,(g) + 16H,S(g) | kJ 6S, (s) + 32H,0(1) 1680, (g) + 32H,S(g) O kJ A mixture of gaseous reactants is put into a cylinder, where a chemical reaction turns them into gaseous products. The 1 atm pressure cylinder has a piston that moves in or out, as necessary, to keep a constant pressure on the mixture of 1 atm. The cylinder is also submerged in a large insulated water bath. (See sketch at right.) piston cylinder From previous experiments, this chemical reaction is known to absorb 170. kJ of energy. water bath gases The position of the piston is monitored, and it is determined from this data that the system does 220. kJ of work on the piston during the reaction. exothermic Is the reaction exothermic or endothermic? x10 endothermic Does the temperature of the water bath go up or down? dn down neither in Does the piston move in or out? out neither in Does heat flow into or out of the gas mixture? out neither How much heat flows? Be sure your answer has the correct number of significant digits. | kJ

The balanced combustion reaction for C,H, is 2 C,H,(1) + 15 O,(g) 12 CO, (g) + 6 H, O(1) + 6542 kJ If 8.700 g C,H, is burned and the heat produced from the burning is added to 5691 g of water at 21 °C, what is the final 9. temperature of the water?

The heater used in a 4.32 m×3.69 m×3.01 m4.32 m×3.69 m×3.01 m dorm room uses the combustion of natural gas (primarily methane gas) to produce the heat required to increase the temperature of the air in the dorm room. Assuming that all of the energy produced in the reaction goes towards heating only the air in the dorm room, calculate the mass of methane required to increase the temperature of the air by 5.30 °C5.30 °C. Assume that the specific heat of air is 30.0 J/K·mol30.0 J/K·mol and that 1.00 mol1.00 mol of air occupies 22.4 L22.4 L at all temperatures. Enthalpy of formation values can be found in this table. Assume gaseous water is produced in the combustion of methane.

A mixture of gaseous reactants is put into a cylinder, where a chemical reaction turns them into gaseous products. The cylinder has a piston that moves in or out, as necessary, to keep a constant pressure on the mixture of 1 atm. The cylinder is also submerged in a large insulated water bath. (See sketch at right.) 1 atm pressure pist From previous experiments, this chemical reaction is known to absorb 278. kJ of energy. The temperature of the water bath is monitored, and it is determined from this data that 285. kJ of heat flows into the system during the reaction. gases O exothermic Is the reaction exothermic or endothermic? O endothermic O up Does the temperature of the water bath go up or down? O down O neither in Does the piston move in or out? O out O neither O does work Does the gas mixture do work, or is work done on it? O work is done on it O neither How much work is done on (or by) the gas mixture? Round your answer to 1 significant digit.

A 140-g aluminum cylinder is removed from a liquid nitrogen bath, where it has been cooled to - 196∘C . The cylinder is immediately placed in an insulated cup containing 90.0 g of water at 15.0 ∘C . If your answer is 0 ∘C , determine the amount of water that has frozen.

A coin dealer, offered a rare silver coin, suspected that it might be a counterfeit nickel copy. The dealer heated the coin, which weighed 14.5 g to 100°C in boiling water and then dropped the hot coin into 25.0 g of water at T = 15.0°C in an insulated coffee-cup, and measured the rise in temperature. If the coin was really made of silver, what would the final temperature of the water be (in °C)? (for nickel, s = 0.445 J/g°C; for silver, s = 0.233 J/g°C )

3 A hot air balloon will lie flat until a heat source is initiated, Once enough heat is produced the balloon begins to inflate. What process is responsible for a hot air bailloon's inflation? Thermal energy will cause hydrogen in A the air to change into helium, which causes the balloon to inflate, Thermal energy from the heat source will B heat the fabric of the balloon, which causes the balloon to inflate. Thermal energy will move from the surrounding air to the heat source which causes air to sink into the balloon, which causes the balloon to inflate. Thermal energy will move from the heat source to surrounding cooler air which causes the air to rise until uniform temperature has been reached, which causes the balloon to inflate.

Please help me answer this thermochemistry question (i keep getting it wrong and this is my last try )

A 10.7 g sample of aluminum at 85.3 0C is added to 117 mL of water initially at 14.6 0C. Assuming no heat is lost to the surroundings, calculate the final temperature of the system.

Chaeyoung wants to study the heat transfer between a 50 g of heated block of iron (cFe = 0.449 J/g ⁰C) at 500 ⁰C and 100 g of water (cH2O = 4.184 J/g ⁰C) at 10 ⁰C using a calorimeter. Find qH2O and qFe.