Calculate the total heat in kJ required to raise the temperature of 25.0 g of solid ethanol at -135.0 °C to liquid at 72.0 °C. (Give the final answer in kJ.) kJ = b

The specific heat capacity of liquid bromine is 0.226 J g^−1 K^−1. How much heat is required to raise the temperature of 31.2 g of bromine from 25.00 °C to 27.30 °C?

Ethylene glycol (specific heat 2.42 J/g°C) is used as a coolant in automotive engines. Calculate the energy released (q) when 3.65 kg of ethylene glycol is cooled from 132 °C to 85 °C.

The temperature of a sample of iron increased by 22.0 °C22.0 °C when 269 J269 J of heat was applied. What is the mass of the sample?   Substance Specific heat J/(g · °C) lead 0.128 silver 0.235 copper 0.385 iron 0.449 aluminum 0.903

Aluminum metal can be produced by reducing solid aluminum oxide (Al2O3) with carbon (graphite). Carbon monoxide is the other product. What is the enthalpy change (AH° in kJ) when 25.0 g of aluminum metal is produced in this manner? You will need to balance the chemical equation. Enthalpies of formation (in kJ mol¯¹): Al2O3(s) -1675.7 CO(g) -110.5 Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a -623 b 623 с -734 d 734

When 2.50 g of sodium hydroxide (NaOH) was dissolved in 150.00 g of water a value of 10.50oC was obtained for ΔT. Calculate the value (calories) for the heat of solution of 2.50 g of NaOH. Calculate the number of calories that would be produced if one mole of sodium hydroxide was dissolved. (ΔHsolnNaOH)

Determine the reaction enthalpy, ΔHrxn for the reaction, N2H4(l) + CH4O(l) → CH2O(g) + N2(g) + 3H2 (g)   ΔHrxn = ??? kJ by using some combination of the reactions below. 1) 2NH3(g) → N2H4(l) + H2(g) ΔH1 = 20 kJ 2) 2NH3(g) → N2(g) + 3H 2(g) ΔH2 = 60 kJ 3) CH2O(g) + H2(g) → CH 4O(l) ΔH3 = 80 kJ.              .

The molar heat of solution of a substance is found to be +21.38 kJ/mol. The addition of 0.100 mol of this substance to 1.000L of water initially at 40.0 degrees celsius results in a temperature decrease. Assume the specific heat of the resulting solution to be equal to that of pure water. Find the final temperature of the solution (Also assume that the heat capacity of the calorimeter is negligible).

A hot lump of 37.137.1 g of iron at an initial temperature of 95.6 °C95.6 °C is placed in 50.0 mL H2OH2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the iron and water, given that the specific heat of iron is 0.449 J/(g·°C)?0.449 J/(g·°C)? Assume no heat is lost to surroundings.