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1 year ago

What is the pH of a solution with (H+) =2.3x10 -6

Chemistry

1 answer:

castortr0y [4]1 year ago

5 0

P
H
=
−
log
10
[
H
3
O
+
]
=
−
log
10
{
2.3
×
10
−
6
}
=
−
{
−
5.64
}
=
5.64

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How many grams of H 2O are produced from 28.8 g of O 2? (Molar Mass of H 2O = 18.02 g) (Molar Mass of O 2=32.00 g) 4 NH 3 (g) +

krek1111 [17]

Answer: 13.9 g of $H_2O$ will be produced from the given mass of oxygen

Explanation:

To calculate the moles :

$\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}$

$\text{Moles of} O_2=\frac{28.8g}{32.00g/mol}=0.900moles$

The balanced chemical reaction is:

$4NIO_2(g)+7O_2(g)\rightarrow 4NO_2(g)+6H_2O(g)$

According to stoichiometry :

7 moles of $O_2$ produce = 6 moles of $H_2O$

Thus 0.900 moles of $O_2$ will produce = $\frac{6}{7}\times 0.900=0.771moles$ of $H_2O$

Mass of $H_2O=moles\times {\text {Molar mass}}=0.771moles\times 18.02g/mol=13.9g$

Thus 13.9 g of $H_2O$ will be produced from the given mass of oxygen

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2 years ago

Explain electronegativity and how it relates to both molecular and ionic bonding.

Keith_Richards [23]

Answer:

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2 years ago

A chemical reaction can theoretically produce 137.5 grams of product, but in actuality 112.9 grams are

Butoxors [25]

<h3>Answer:</h3>

82.11%

<h3>Explanation:</h3>

We are given;

Theoretical mass of the product is 137.5 g
Actual mass of the product is 112.9 g

We are supposed to calculate the percentage yield

We need to know how percentage yield is calculated;
To calculate the percentage yield we get the ratio of the actual mass to theoretical mass and express it as a percentage.

Thus;

% yield = (Actual mass ÷ Experimental mass) × 100%

= (112.9 g ÷ 137.5 g) × 100%

= 82.11%

Therefore, the percentage yield of the product is 82.11 %

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2 years ago

Identify the following changes as physical or chemical.

andrezito [222]

Answer:

physical

Explanation:

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2 years ago

Molarity is measured in

aniked [119]

Answer D moles per L

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2 years ago