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Find the total energy involved in converting 450.0g of water from -21°C to 35°C. Hvan Water = 40.7 KJ/mol Hrus Water = 6.01 KJ/mol Solid C =2.03 J/g°C water Liquid Cwater =4.184 J/g°C Gas Cwater 2.01 J/g°C O 235 KJ O 150 KJ O 85 KJ 255 KJ

I just want to verify if my answer is correct.

Can you help me? 4. How much energy is removed from 500.0 g of water when the temperature is lowered by 1.10 o C? Answer: -550. cal (or -2.30 x 103 J) 5. How much energy is required to raise the temperature of 1000.0 g of water from 23.00 o C to 26.00 o C? Answer: 3.00 x 103 cal (or 1.26 x 104 J) 6. The specific heat of copper is (0.0924 cal/go C), how much energy is required to raise the temperature of 10.0 g of copper by 100.0 o C? Answer: 92.4 cal

ab The enthalpy of solution (AH) of NaNO3 is 20.4 kJ/mol. If 8.50 g NaNO3 is dissolved in enough water to make a 100.0 mL solution, what is the change in temperature (°C) of the solution? (The specific heat capacity of the solution is 4.184 J/g °C and the density of the solution is 1.02 g/mL). Tap here or pull up for additional resources 1 Q @ 2 W # 3 E $ 4 R % 5 T Question 1 of 10 6 Y & 7 U 8 1 9 1 4 7 +/- 0

When ammonia reacts with dinitrogen oxide gas (ΔHf° = 82.05 kJ/mol), liquid water and nitrogen gas are formed. How much heat (in kJ) is liberated or absorbed by the reaction that produces 365 mL of nitrogen gas at 25°C and 743 mm Hg?   ΔHf° (kJ/mol) NH3(g) –46.1 H2O(l) –285.8 N2(g) 0 N2O(g) 82.05

From this reaction 2NO(g) + 2H₂(g) à N₂(g) + 2H₂O(1), NO H2 N2 Sᵒ (J/mol K) 75.10 191.5 192.3 ΔΗ°f (kJ/mol) -283.74 0 0 What is the standard enthalpy of reaction (AHrnx)? H20 189.0 -373.57

Damp clothes can prove fatal when the outdoor temperature drops (e.g. death by hypothermia). If the clothes you are wearing absorb 94.2 g of water and then dry in a cold wind on Optimist Hill, how much heat (in kJ) would your body lose during the process? (Co H20 = 75.3 J/mol°C and AHvap.H20= 40.81 kJ/mol) (Answer to 1 decimal place) Type your answer.. Next Previous

1. Based from the thermochemical equation given, O2(9) N2(9) + NO2(9) Calculate the heat associated with the decomposition of 2.75 g of NO2(g) ----> AH = +67.6 kJ Is the reaction exothermic or endothermic?