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3 years ago

2 NaOH (s) + CO2(g) → Na2CO3 (s) + H20 (I) How many grams of water can be produced with 1.85 moles of NaOH

Chemistry

2 answers:

maks197457 [2]3 years ago

7 0

Answer:

16.65 grams of water can be produced with 1.85 moles of NaOH.

Explanation:

Mole ratio of NaOH to H2O = 2 : 1

Number of moles of water = (1/2)×1.85= 0.925 moles

Molar mass of water (H2O) = 18g/mol

Mass of the right water = 18g/mol×0.925 mol=16.65 grams

Romashka [77]3 years ago

4 0

Explanation:

Mole ratio of NaOH to H2O = 2 : 1

Moles of H2O = 1.85mol * (1/2) = 0.925mol.

Mass of H2O = 0.925mol * (18g/mol) = 16.65g.

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3 years ago

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Characteristics outlined below

Explanation:

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3 years ago

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Mariulka [41]

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where XY is the salt

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3 years ago

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The balloon in the previous problem will burst if its volume reaches 400. L. Given the initial conditions specified in that prob

NARA [144]

This is an incomplete question, here is complete question.

A metrological balloon contains 250 L of He at 22 C and 740 mmHg.

The balloon in the previous problem will burst if its volume reaches 400 L. Given the initial conditions specified in that problem, at what temperature, in degrees Celsius, will the balloon burst if its pressure at that bursting point is 0.475 atm.

Answer : The final temperature will be, $-44.4^oC$

Explanation :

Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.

The combined gas equation is,

$\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$

where,

$P_1$ = initial pressure of gas = 740 mmHg = 0.974 atm

$P_2$ = final pressure of gas = 0.475 atm

$V_1$ = initial volume of gas = 250 L

$V_2$ = final volume of gas = 400 L

$T_1$ = initial temperature of gas = $22^oC=273+20=293K$

$T_2$ = final temperature of gas = ?

Now put all the given values in the above equation, we get:

$\frac{0.974atm\times 250L}{293K}=\frac{0.475atm\times 400L}{T_2}$

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4 years ago

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8_murik_8 [283]

Answer:

a. positive

b. negative

c. positive

d. negative

Explanation:

In a exothermic reaction, heat is written as a product (del H is negative), whereas in an endothermic reaction heat is written on the reaction side (del H is positive).

For a, it is endothermic process. We know this because to go from solid to liquid you need to put energy into the system. When we put energy into a chemical system it is said to be an endothermic reaction.

For b, it is exothermic reaction. This is because you have to lose the extra energy to go from less ordered states (gas) to more ordered state (liquid). Gas is less ordered because its molecules are freely moving and such. Another way of thinking about this question is just putting the heat on product side and think if I was going in reverse direction I would put heat in product because I would need to add heat to liquid to turn to gas (and if heat is added to product side we know its exothermic). Two ways of thinking whichever you prefer.

The rest have similar explaination.

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4 years ago

2 NaOH (s) + CO2(g) → Na2CO3 (s) + H20 (I) How many grams of water can be produced with 1.85 moles of NaOH​

2 NaOH (s) + CO2(g) → Na2CO3 (s) + H20 (I) How many grams of water can be produced with 1.85 moles of NaOH