<h3>
Answer:</h3>
0.90J/g°C
<h3>
Explanation:</h3>
We are given:
Mass of Aluminium = 10 g
Quantity of heat = 677 Joules
Change in temperature = 125°C - 50°C
= 75°C
We are required to calculate the specific heat capacity of Aluminium
But, Quantity of heat = Mass × specific heat × Change in temperature
Q = mcΔt
Rearranging the formula;
c = Q ÷ mΔt
= 677 J ÷ (10 g × 75°C)
= 677 J ÷ 750g°C
= 0.903 J/g°C
= 0.90J/g°C
Thus, the specific heat capacity of Aluminium is 0.90J/g°C
Answer:
Mass = 20,000 g
Explanation:
Given data:
Mass of MgO formed = ?
Mass of Mg react = 12 Kg (12 Kg × 1000/1 Kg = 12000 g)
Solution:
Chemical equation:
2Mg + O₂ → 2MgO
Number of moles of Mg:
Number of moles = mass/molar mass
Number of moles = 12000 g/ 24 g/mol
Number of moles = 500 mol
Now we will compare the moles of Mg and MgO.
Mg : MgO
2 : 2
500 : 500
Mass of MgO:
Mass = number of moles × molar mass
Mass = 500 mol × 40 g/mol
Mass = 20,000 g
Answer: C) The mass stays constant as it changed from a liquid to a gas
Explanation: Mass stays constant, it's never destroyed or created. It follows the law of conservation of mass.
Im pretty sure it would also be 25
