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3 years ago

A gas at constant volume has a pressure of 3.20 atm at 300. K. What will be the pressure of the gas at 290. K?

Chemistry

1 answer:

melomori [17]3 years ago

3 0

From the general law of gases: PV = nRT,

where P is the pressure (atm),

V is the volume (L),

n is the number of moles,

R is the general gas constant (8.314 L.atm/mol.K),

T is the temperature in Kelvin

at constant volume of the gas: P1T2 = P2T1

P1 = 3.20 atm, T1 = 300 K, T2 = 290 K, P2 = ??

(3.20 atm)(290 K) = P2(300 K)

P2 = (3.20 atm)(290 K)/ (300 K) = 3.093 atm

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2 years ago

Give the SI base unit of each of these quantities. Enter the abbreviation rather than the name of the unit. mass: __________--le

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4 years ago

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brainly.com/question/24944271?

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3 years ago

The specific heat capacity (c) of a substance is the thermal energy required

Ierofanga [76]

Temperature of the same cup of water will rise by 6 °C unless it boils.

<h3>Explanation</h3>

$Q = c\cdot m \cdot \Delta T$ .

However, neither $c$ nor $m$ is given.

Adding $Q = 125\;\text{kJ}$ to this cup of water of mass $m$ rises its temperature by $\Delta T = 1 \; \textdegree{}\text{C}$ .

In other words,

$\begin{array}{lll}Q &=& c \cdot m \cdot \Delta T\\125\;\text{kJ} &=& c \cdot m \times (1 \; \textdegree{}\text{C})\end{array}$

$c \cdot m = \dfrac{Q}{\Delta T} = \dfrac{125\; \text{kJ}}{1 \; \textdegree{}\text{C}}$ .

Both $c$ and $m$ are constant for the same cup of water unless the water boils. It's possible to reuse the value of $c \cdot m$ in the second calculation. Here's how:

$\Delta T = \dfrac{Q}{c\cdot m} = \dfrac{750 \; \text{kJ}}{\dfrac{125\;\text{kJ}}{1\;\textdegree{}\text{C}}} = \dfrac{750}{125} \; \textdegree{}\text{C}} = 6 \; \textdegree{}\text{C}}$ .

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3 years ago