Table of Contents

## How do you calculate heat absorbed by copper?

Explanation:

- E=m⋅C⋅ΔT.
- The mass is =5.82kg.
- The specific heat of copper is C=0.385kJkg−1ºC−1.
- ΔT=328.3−21.5=306.8.
- E=5.82⋅0.385⋅306.8=687.4kJ.

**How do you calculate the amount of heat absorbed?**

The heat absorbed is calculated by using the specific heat of water and the equation ΔH=cp×m×ΔT. 4. Water is vaporized to steam at 100oC. The heat absorbed is calculated by multiplying the moles of water by the molar heat of vaporization.

**How do I calculate specific heat?**

How do I calculate specific heat? Q = m*s*dT, where Q = heat, m = mass, s = specific heat, and dT is the change in temperature (T2 – T1). You can use this formula to calculate the specific heat. In the case of gases, just replace the mass by moles of the gas.

### How do you calculate the heat required to raise the temperature?

Specific heat is the amount of heat required to raise one gram of any substance one degree Celsius or Kelvin. The formula for specific heat is the amount of heat absorbed or released = mass x specific heat x change in temperature.

**How much heat must be absorbed by 375 g to raise its temperature by 25 C?**

Answer: 39.2 kJ.

**What is the specific heat of copper?**

0.385

Heat Capacities for Some Select Substances

Substance | specific heat capacity Cp,s (J/g °C) | molar heat capacity Cp,m (J/mol °C) |
---|---|---|

copper | 0.385 | 24.47 |

granite | 0.790 | — |

graphite | 0.710 | 8.53 |

helium | 5.1932 | 20.786 |

## How much heat must be absorbed by 375 grams of water to raise its temperature by 25 C?

**How much heat was absorbed by the calorimeter?**

The heat absorbed by the calorimeter is q1 = 534 J/°C × (26.9 °C – 23.4 °C) = 1869 J. The heat absorbed by water is q1 = 675 mL × 0.997 g/mL × 4.184 J/g °C × (26.9 °C – 23.4 °C) = 9855 J. The overall amount of heat q = q1 + q1 = 11,724 J or 11.7 kJ with three significant digits.

**When 56 J of heat are added to 11 g of a liquid its temperature rises from 10.4 C to 12.7 C What is the heat capacity of the liquid?**

2.2 J/ g∘C.

### What is the heat required to raise the temperature of 1g?

The calorie is defined as the amount of energy (heat) needed to increase the temperature of one gram of water by 1°C. The SI energy unit is the joule. 1 Calorie = 4.186 joule. The heat required would be 4.018 J.

**How much heat did the water absorb?**

One of water’s most significant properties is that it takes a lot of energy to heat it. Precisely, water has to absorb 4,184 Joules of heat (1 calorie) for the temperature of one kilogram of water to increase 1°C. For comparison sake, it only takes 385 Joules of heat to raise 1 kilogram of copper 1°C.

**What is the specific heat of lead in J GC?**

0.159

Specific Heats (Csp)

Substance | Formula | Csp (J/goC) |
---|---|---|

Lead | Pb | 0.159 |

Magnesium | Mg | 1.017 |

Mercury | Hg | 0.138 |

Neon | Ne | 1.03 |