The specific beta in aluminum is 0,900 J/g • Celsius. How much heat is required to raise the temperature of a 30.0 g block of aluminum from 25 degrees celsius to 75 degrees celsius

1350J

Explanation:

Heat energy = ?

Mass = 30.0g

Specific heat capacity (c) = 0.90J/g°C

Initial temperature (T1) = 25°C

Final temperature (T2) = 75°C

Heat energy (Q) = mc∇T

Q = heat energy

M = mass of the substance

C = specific heat capacity of the substance

∇T = change in temperature of the substance = T2 - T1

Q = mc∇T

Q = 30 × 0.90 × (75 - 25)

Q = 27 × 50

Q = 1350J

The heat energy required to raise the temperature of the metal from 25°C to 75°C is 1350J

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