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2 years ago

I have 0.92 moles of water (H20). What is the mass of the water?

Chemistry

1 answer:

strojnjashka [21]2 years ago

5 0

Ans:

16.57 g

Explanation:

If you have 0.92 moles of water you would take your moles and multiply it by its molar mass (18.01528 g/mol) to find your specific mass.

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44.2124+0.81+7.335 significant digits

zhenek [66]

Explanation:

We need to understand and apply the rules of significant figures when carrying out addition operations to solve this problem:

Rules of significant figures:

Non-zero digits are always significant in a given number
Any zeros between two significant digits are significant.
A final zero or trailing zeros in the decimal portion is significant.
Any leading zero in a decimal is significant.

In addition, the answer of the sum is given to the least number of significant digits of the given numbers:

44.2124

+ 0.81

+ 7.335

sum 52.3574

Now the least number of significant figure is 2 as seen in 0.81

we round the sum up to 52

learn more:

Significant numbers brainly.com/question/6384538

#learnwithBrainly

4 0

2 years ago

The following reaction was carried out in a 3.00 L reaction vessel at 1100 K:

Nady [450]

Answer:

$Q=0.840$

Explanation:

Hello,

In this case, since the given undergoing chemical reaction is correctly balanced, the reaction quotient is computed as well as the equilibrium constant but in terms of the given concentrations that are:

$C_{C}=\frac{5.25mol}{3.00L} =1.75M\\C_{H_2O}=\frac{12.2mol}{3.00L} =4.07M\\C_{CO}=\frac{3.90mol}{3.00L}=1.30M\\C_{H_2}=\frac{7.90mol}{3.00L} =2.63M$

In such a way, the reaction quotient turns out:

$Q=\frac{C_{CO}C_{H_2}}{C_{H_2O}}=\frac{1.30M*2.63M}{4.07M}\\ Q=0.840$

Taking into account that carbon is not included since it is solid.

Best regards.

7 0

2 years ago

How much energy is released when 18.0 g of water at 0°C changes from liquid to solid?

yaroslaw [1]

I love you too funny I love you too

7 0

2 years ago

What allows nutrients to enter Plants and animals are able to be transported

elena55 [62]

I think it’s the cell membrane if you’re talking about animal cells and plant cells.

3 0

3 years ago

Octane has a density of 0.703 g/ml. Calculate the mass of CO2(g) produced by burning one

STatiana [176]

The mass of CO₂ gas produced during the combustion of one gallon of octane is 8.21 kg.

The given parameters:

Density of the octane, ρ = 0.703 g/ml
Volume of octane, v = 3.79 liters

The mass of the octane burnt is calculated as follows;

$m = \rho V\\\\m = 0.703 \ \frac{g}{ml} \times 3.79 \ L \ \frac{1000 \ ml}{L} \\\\m = 2,664.37 \ g$

The combustion reaction of octane is given as;

$2C_8H_{18} + \ 25O_2 \ --> \ 16CO_2 \ + \ 18H_2O$

From the reaction above:

228.46 g of octane -------------------> 704 g of CO₂ gas

2,664.37 of octane --------------------> ? of CO₂ gas

$= \frac{2,664.37 \times 704}{228.46} \\\\= 8,210.3 \ g\\\\= 8.21 \ kg$

Thus, the mass of CO₂ gas produced during the combustion of one gallon of octane is 8.21 kg.

Learn more about combustion of organic compounds here: brainly.com/question/13272422

8 0

2 years ago

I have 0.92 moles of water (H20). What is the mass of the water?​

I have 0.92 moles of water (H20). What is the mass of the water?