At constant pressure, the amount of heat required to increase the temperature of 1g substance to 1oC is calculated by the formula-
Q = m * C × ΔT
Where Q = amount of heat required
m = mass of substance
C = specific heat
ΔT = change in temperature = final temperature – initial temperature
Now putting the given values
m = 45 g
C = specific heat for water = 4.186 J/ goC
final temperature = 143.0oC
initial temperature = - 10.0oC
So ΔT = 143.0oC - (- 10.0oC )
= 153.0oC
Now putting the values-
Q = m * C × ΔT
Q = 45 g * 4.186 J/ goC × 153.0oC
= 28820.61 J
Q = 28.821 kJ
V Hint Check Answer Question 14 of 16 > At 1 atm, how much energy is...
Question 15 of 22 > Attempt 8 At 1 atm, how much energy is required to heat 710 g H, 0(s) at -12.0 C to H,O(g) at 119.0 'C? Use the heat transfer constants found in this table. q=38 kJ
At 1 atm, how much energy is required to heat 83.0 g H,O(s) at -10.0°C to H, O(g) at 141.0 °C? Use the heat transfer constants found in this table.
At 1 atm, how much energy is required to heat 93.0 g H2O(s)93.0 g H2O(s) at −10.0 ∘C−10.0 ∘C to H2O(g)H2O(g) at 137.0 ∘C?137.0 ∘C? Use the heat transfer constants found in this table.
At 1 atm, how much energy is required to heat 71.0 g of H2O(s) at − 20.0 °C to H2O(g) at 171.0 °C? Heat transfer constants can be found in this table.
At 1 atm, how much energy is required to heat 75.0 g H2O(s) at −22.0 ∘C to H2O(g) at 147.0 ∘C? Use the heat transfer constants found in this table.
At 1 atm, how much energy is required to heat 73.0 g H2O(s) at −14.0 ∘C to H2O(g) at 123.0 ∘C? Use the heat transfer constants found in this table.
At 1 atm, how much energy is required to heat 75.0 g H2O(s) at -14.0°C to H2O(g) at 119.0 °C? Use the heat transfer constants found in this table.
At 1 atm, how much energy is required to heat 79.0 g of H0(s) at-24.0 "C to H,0(g) at 1670 "C? Helpful constants can be found bere kJ
1. At 1 atm, how much energy is required to heat 35.0 g H2O(s) at −10.0 ∘C to H2O(g) at 137.0 ∘C? Use the heat transfer constants found in this Quantity per gram per mole Enthalpy of fusion 333.6 J/g 6010. J/mol Enthalpy of vaporization 2257 J/g 40660 J/mol Specific heat of solid H2O (ice) 2.087 J/(g·°C) * 37.60 J/(mol·°C) * Specific heat of liquid H2O (water) 4.184 J/(g·°C) * 75.37 J/(mol·°C) * Specific heat of gaseous H2O (steam) 2.000...
At 1 atm, how much energy is required to heat 67.0 g H2O(s)67.0 g H2O(s) at −10.0 ∘C−10.0 ∘C to H2O(g)H2O(g) at 175.0 ∘C?175.0 ∘C?