A 436.3 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 °C to 147.6 °C. (heat capacity of liquid = 1.62 J/g･°C; heat capacity of gas = 1.04 J/g･°C; ∆Hvap = 78.11 kJ/mol; Tb = 160.3 °C)   a) How much energy (in KJ) is absorbed/released to cool the gas?   b) How much energy (in kJ) is absorbed/released to condense the gas?   c) How much energy (in KJ) is absorbed/released to cool the liquid?   d) What is the total amount of energy that must be absorbed/released for the entire process?

muny giallis Of CU, are produced per 2.50 x 103 kJ of heat released? 0.0809 g 3.56g 31.3 g 157 g 309g average home in Colorado requires 20. GJ of heat per month. How many grams of natural gas (methane) must be burned to supply this energy? CH.(g) + 20:(g)→CO.(g) + 2H,0(1) AH°=-890.4 kJ/mol 1.4 x 10 g 3.6x 10° g 7.1 x 10 g 2.2 x 10 g 1.4x 10' g 46.An A) в) C) D) E) 47.Given the thermochemical equation 2SO2(g) + O(g)→2SO:(g), AH°r=-198 kJ/mol, how much heat is evolved when 600. g of SO, is burned? 5.46 x 10 kJ A) в) C) 928 kJ 1.85 x 10 kJ 59,400 kJ 3.71 x 10 kJ D) E) 48. Determine the heat given off to the surroundings when 9.0g of aluminum reacts according to the equation 2AI + Fe,O,Al,O;+ 2Fe, AH°, n-849 kJ/mol

A substance, X, has the following properties. (Size of mass is 250. g.) Specific Heat Capacities ΔΗvap 20. kJ/mol C(s) 3.0 J/g.°C AHfus 5.0 kJ/mol C(I) 2.5 J/g.°C bp 75°C C(g) 1.0 J/g.°C mp -15°C Calculate the energy that must be removed to convert substance X from a gas at 124°C to a solid -50.5°C. Assume X has a molar mass of 75.0 g/mol.

How much heat is transferred from a 4.00 g gold nugget (specific heat = 0.129 J/g-°C) initially at 45.4°C when it is dropped into 5 kg of water (specific heat = 4.184 J/g-°C) initially at 25.0°C?

A 46.81 g46.81 g sample of a substance is initially at 25.7 °C.25.7 °C. After absorbing 1415 J1415 J of heat, the temperature of the substance is 177.9 °C.177.9 °C. What is the specific heat (?) of the substance?

Tautomers are constitutional isomers that differ in the location of adouble bond and a hydrogen atom. Two tautomers are in equilibriumwith each other. Explain this ?

Steam can cause more severe burns than water, even if both are at the same temperature. Calculate the amount of heat releasedfrom 93 g of steam at 100.0°C as it cools to 37°C (body temperature), and the amount of heat released from 93 g of water at 100.0 °Cas it cools to 37 °C. The AHvaporization of water is 43.9 kJ mol'1 and the specific heat of water is 4.184 J g'1°C-].The heat content of 93 g of water at 100°C cooling to 37°C isThe heat released when 93 g of water vapor at 100°C cools to 37°C iskJ.

How much heat in Joules must be used to raise the temperature of 0.340 kg of water from 28oC to 98oC? (heat of water is 4.18 J/(g-oC).

Can this be explained step by step

A 1.25-g chunk of sodium metal is cautiously dropped into a mixture of 50.0 g water and 50.0 g ice, both at 0°C. The reaction is 2Na(s) + 2H₂O(1)→ 2NaOH(aq) + H₂(g) AH = -368 kJ Assuming no heat loss to the surroundings, will the ice melt? v Assuming the final mixture has a specific heat capacity of 4.18 J/g °C, calculate the final temperature. The enthalpy of fusion for ice is 6.02 kj/mol. Temperature=