2 years ago

Calculate the mass of magnesium oxide that is produced when 64 g of magnesium is combined with 1.32 g of oxygen

1 answer:

3 0

64 + 1.24 = 65.24 g of MgO

You might be interested in

Nuetrik [128]

Answer:

Explanation:

triple beam balance

sorry if i am wrong! can be brainliest?

5 0

2 years ago

iragen [17]

the answer is in the picture, btw the molar mass for the first one is wrong, it should be 77.98, and the final product is 2.32

6 0

3 years ago

Blababa [14]

2 stands for valency of ca ion

its +2

that it takes two electrons to complete its shell

8 0

2 years ago

nirvana33 [79]

Answer: An atom

Hope this helps!

8 0

11 months ago

shusha [124]

Answer: The enthalpy of combustion, per mole, of butane is -2657.4 kJ

Explanation:

The balanced chemical reaction is,

$2C_4H_{10}(g)+13O_2(g)\rightarrow 8CO_2(g)+10H_2O(g)$

The expression for enthalpy change is,

$\Delta H=[n\times H_f_{products}]-[n\times H_f_{reactants}]$

Putting the values we get :

$\Delta H=[8\times H_f_{CO_2}+10\times H_f_{H_2O}]-[2\times H_f_{C_4H_{10}+13\times H_f_{O_2}}]$

$\Delta H=[(8\times -393.5)+(10\times -241.82)]-[(2\times -125.7)+(13\times 0)]$

$\Delta H=-5314.8kJ$

2 moles of butane releases heat = 5314.8 kJ

1 mole of butane release heat = $\frac{5314.8}{2}\times 1=2657.4kJ$

Thus enthalpy of combustion per mole of butane is -2657.4 kJ

3 0

2 years ago