All categories

2 years ago

Write a complete, balanced equation for the following reactions:

Chemistry

1 answer:

lys-0071 [83]2 years ago

6 0

Answer:

Solution given:

c) Magnesium metal plus silver acetate (teachers note:

Balanced chemical equation:

$\boxed{\bold{\green{Mg+AgC_{2}H_{3}O_{2}\rightarrow MgC_{3}H_{3}O_{2}+Ag^{+}}}}$

d) hydrobromic acid plus zinc metal (teachers note:

Balanced chemical equation:

$\boxed{\bold{\green{2HBr+Zn \rightarrow Be_{2}+H_{2}}}}$

You might be interested in

A _____ speeds up a chemical reaction, but is not directly involved in the reaction.

igomit [66]

I think your answer is nunclear.

4 0

3 years ago

Read 2 more answers

How much energy does it take to melt 2 kg of ice? (Refer to table of constants for water.)

ioda

It would be C

2 kg x 1000 g/kg x 1mol/18.02 x 6.03 kj/mol = 669kj

5 0

2 years ago

Read 2 more answers

Which action by the British government was

Lera25 [3.4K]

The answer is (4) taxing the colonies without representation in Parliament

This set off the Revolutionary War, and the slogan "no taxation without representation" became famous.

3 0

3 years ago

Millions of years ago in many different regions of the world, large-scale burials of organic matter were followed by the formati

kramer

The answer is A: Areas where the geologic process occurred now have major petroleum reserves

5 0

2 years ago

Read 2 more answers

Given the following balanced equation, if the rate of O2 loss is 3.64 × 10-3 M/s, what is the rate of formation of SO3? 2 SO2(g)

Fynjy0 [20]

Answer:

Rate of formation of SO₃ $[\frac{d[SO_{3}] }{dt}]$ = 7.28 x 10⁻³ M/s

Explanation:

According to equation 2 SO₂(g) + O₂(g) → 2 SO₃(g)

Rate of disappearance of reactants = rate of appearance of products

⇒ $-\frac{1}{2} \frac{d[SO_{2} ]}{dt} = -\frac{d[O_{2} ]}{dt}=\frac{1}{2} \frac{d[SO_{3} ]}{dt}$ -----------------------------(1)

Given that the rate of disappearance of oxygen = $-\frac{d[O_{2} ]}{dt}$ = 3.64 x 10⁻³ M/s

So the rate of formation of SO₃ $[\frac{d[SO_{3}] }{dt}]$ = ?

from equation (1) we can write

$\frac{d[SO_{3}] }{dt} = 2 [-\frac{d[O_{2}] }{dt} ]$

⇒ $\frac{d[SO_{3}] }{dt}$ = 2 x 3.64 x 10⁻³ M/s

⇒ $[\frac{d[SO_{3}] }{dt}]$ = 7.28 x 10⁻³ M/s

∴ So the rate of formation of SO₃ $[\frac{d[SO_{3}] }{dt}]$ = 7.28 x 10⁻³ M/s

7 0

2 years ago