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3 years ago

Can yall plz help me it’s a huge major grade and i don’t know how to do this

Chemistry

1 answer:

fomenos3 years ago

3 0

Answer:

1. 48 mols

2. 0.2 M

5. 1.25 L

Explanation:

Molarity= mols divided by liters

Hope this helps not sure about 3 and 4

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Ethylene, a gas found in nature, is commonly used to ripen bananas and other fruits. Which compound is ethylene?

Reika [66]

Answer:

C2H4

Explanation:

cause the compound of ethylene is C2H4

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3 years ago

Question 3 0 / 1 point How many grams of carbon atoms are present in a sample of C3H8 if there are 4.10 moles of hydrogen atoms

hodyreva [135]

Answer:

18.45 g of C

Explanation:

This is a problem of rules of three:

1 mol of C₃H₈ contains 3 moles of C and 8 moles of H

If 8 moles of H are contained in 1 mol of propane

4.10 moles of H are contained in (4.1 . 1) /8 = 0.5125 moles

Now, If 1 mol of propane contains 3 moles of C

0.5125 moles of propane may contain (0.5125 . 3) / 1 = 1.5375 moles of C

Let's convert the moles to mass:

1.5375 mol . 12 g /mol = 18.45 g

5 0

2 years ago

Based on the table, which city was in danger of flooding?

dalvyx [7]

Answer:

I think the answer is Toledo

8 0

2 years ago

Carbon dioxide dissolves in water to form carbonic acid, which is primarily dissolved CO2. Dissolved CO2 satisfies the equilibri

lorasvet [3.4K]

Explanation:

The reaction equation will be as follows.

$CO_{2}(aq) + H_{2}O \rightleftharpoons H^{+}(aq) + HCO^{-}_{3}(aq)$

Calculate the amount of $CO_{2}$ dissolved as follows.

$CO_{2}(aq) = K_{CO_{2}} \times P_{CO_{2}}$

It is given that $K_{CO_{2}}$ = 0.032 M/atm and $P_{CO_{2}}$ = $1.9 \times 10^{-4}$ atm.

Hence, $[CO_{2}]$ will be calculated as follows.

$[CO_{2}]$ = $K_{CO_{2}} \times P_{CO_{2}}$

= $0.032 M/atm \times 1.9 \times 10^{-4}atm$

= $0.0608 \times 10^{-4}$

or, = $0.608 \times 10^{-5}$

It is given that $K_{a} = 4.46 \times 10^{-7}$

As, $K_{a} = \frac{[H^{+}]^{2}}{[CO_{2}]}$

$4.46 \times 10^{-7} = \frac{[H^{+}]^{2}}{0.608 \times 10^{-5}}$

$[H^{+}]^{2}$ = $2.71 \times 10^{-12}$

$[H^{+}]$ = $1.64 \times 10^{-6}$

Since, we know that pH = $-log [H^{+}]$

So, pH = $-log (1.64 \times 10^{-6})$

= 5.7

Therefore, we can conclude that pH of water in equilibrium with the atmosphere is 5.7.

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2 years ago

7.Calculate the volume of nitrogen that reacts with 12dm3 of hydrogen with the volume of both gases measured at rtp:

marta [7]

Answer:

4.03dm³

Explanation:

The reaction expression is given as:

3H₂ + N₂ → 2NH₃

Volume of hydrogen = 12dm³

AT rtp:

1 mole of gas occupies volume of 22.4dm³

x mole of hydrogen will occupy a volume of 12dm³

Number of moles of hydrogen = $\frac{12}{22.4}$ = 0.54mole

From the balanced reaction equation:

3 mole of hydrogen gas combines with 1 mole of Nitrogen gas

0.54 mole of hydrogen as will therefore combine with $\frac{0.54}{3}$ = 0.18moles of nitrogen gas

Since ;

1 mole of gas occupies a volume of 22.4dm³

0.18moles of Nitrogen gas will occupy 0.18 x 22.4 = 4.03dm³

6 0

2 years ago