How many calories of are required to heat 731 grams of water from 35°c to 83°c? (assume that the specific heat of water is 1.00
2 answers:
Answer:
The calories required = 35088
Explanation:
The heat required can be calculated by using specific heat of the water and mass and temperature raised.
The specific heat of water is the amount of heat required to raise the temperature of one gram of water by one degree celsius
Thus
Heat required = mass of water X specific heat X change in temperature
Given:
Specific heat of water = 1 cal /g °C
mass of water = 731 g
change in temperature = 83-35 = 48°C
Putting values
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Answer: Mass of required to form 930 kg of iron is 1328 kg
Explanation:
To calculate the number of moles, we use the equation:
.....(1)
For iron:
Given mass of iron = 930 kg = 930000 g (1kg=1000g)
Molar mass of iron = 56 g/mol
Putting values in equation 1, we get:
The chemical equation for the production of iron follows:
By Stoichiometry of the reaction:
2 moles of iron are produced by = 1 mole of
So, 16607 moles of iron will be produced by = of
Now, calculating the mass of from equation 1, we get:
Mass of =
Thus mass of required to form 930 kg of iron is 1328 kg