If it takes 526 j of energy to warm 7.40g of water by 17 degrees celsius, how much energy would be needed to warm 7.40g of water by 55 degrees celsius?

Heat required = 1702 J

Explanation:

The amount of heat energy (Q) required to raise the temperature of water of mass (m) is given as:

where c = specific heat capacity

ΔT =change in temperature

It is given that:

When ΔT = 17 C, Q = 526 J and m = 7.40 g

i.e.

The amount of heat required to increase the temperature of 7.40 g water by 55 C would be:

the answer is d. 74.02

as given the equation is

2al + 6 hcl > 2 alcl3 + 3 h2(g)

as per equation two moles of aluminum reacts with six moles of hcl to give two moles of alcl3 and three moles of hydrogen gas

given: three moles of al are present and 7 moles of hcl

for three moles of aluminum nine moles of hcl will be required

however as 7 moles of hcl are present so the limiting reagent is hcl

hcl is going to decide the number of moles of product formed

when six moles of hcl are present = 3 moles of h2 are formed

when one mole of hcl is present == 3/6 mole sof h2 will be formed

when 7 moles of hcl are present = 3 x 7/ 6 moles of h2 will be formed = 3.5 moles of h2