Balance the following equations:

1 answer:

7 0

<h2>Hey There!</h2><h2>_____________________________________</h2><h2>Answer:</h2><h2>_____________________________________</h2>

(I) $N_{2} + 3H_{2} --> 2NH_{3}$

(II) $P_{4} + 5O_{2} --> 2P_{2} O_{5}$

(III) $2NaF + Br_{2} -->2NaBr + F_{2}$

(IV) $2ZnS + 3O_{2} --> 2ZnO + 2SO_2$

(V) $Pb(NO_3)_2 + 2NaCl --> 2NaNO_3 + PbCl_2$

<h2>_____________________________________</h2><h2>Best Regards,</h2><h2>'Borz'</h2>

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Answer:

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sample of substance X has a mass of 326.0 g releases 4325.8 cal when it freezes at its freezing point. If substance X has a mola

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Number of moles ( substance x ):

1 mole --------- 58.45 g/mol
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3 years ago

Read 2 more answers

A 256 mL sample of HCl gas is in a flask where it exerts a force (pressure) of 67.5 mmHg. What is the pressure of the gas if it

Effectus [21]

Answer:

The pressure in the new flask would be $128\; \rm mmHg$ if the $\rm HCl$ here acts like an ideal gas.

Explanation:

Assume that the $\rm HCl$ sample here acts like an ideal gas. By Boyle's Law, the pressure $P$ of the gas should be inversely proportional to its volume $V$ .

For example, let the initial volume and pressure of the sample be $V_1$ and $P_1$ . The new volume $V_2$ and pressure $P_2$ of this sample shall satisfy the equation: $P_1 \cdot V_1 =P_2 \cdot V_2$ .

In this question,

The initial volume of the gas is $V_1= 256\; \rm mL$ .
The initial pressure of the gas is $P_1 = 67.5\; \rm mmHg$ .
The new volume of the gas is $V_2 = 135\; \rm mL$ .

The goal is to find the new pressure of this gas, $P_2$ .

Assume that this sample is indeed an ideal gas. Then the equation $P_1 \cdot V_1 =P_2 \cdot V_2$ should still hold. Rearrange the equation to separate the unknown, $P_2$ . Note: make sure that the units for $V_1$ and $V_2$ are the same before evaluating. That way, the unit of

$\begin{aligned} & P_2\\ &= \frac{P_1 \cdot V_1}{V_2} \\ &= \frac{256\; \rm mL \times 67.5\; \rm mmHg}{135\; \rm mL} \\ & \approx 128\; \rm mmHg\end{aligned}$ .