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3 years ago

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3. A sample of air in a syringe exerts a pressure of 1.02 atm at 22.0°C. The syringe is placed in a boiling-water bath at 100.0°

C. The
pressure is increased to 1.23 atm by pushing the plunger in, which reduces the volume to 0.224ml What was the initial volume?

1 answer:

inysia [295]3 years ago

8 0

Answer:

0.214 mL

explanation:

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Give the chemical symbol for the element with the ground‑state electron configuration [ Ar ] 4 s 2 3 d 1 . symbol: Determine the

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Answer:

Sc (Scandium) has the given electronic configuration.

Explanation:

The given electronic configuration is [Ar] $4s^{2}3d^{1}$ .

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For 4s subshell

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Note:

l values for subshells:

s : 0

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How much energy is required to raise the temperature of 10.6 grams of gaseous neon from

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Answer:

Approximately $1.95 \times 10^{2}\; \rm J$ .

Explanation:

Look up the specific heat of gaseous neon:

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Calculate the required temperature change:

$\Delta T = (37.9 - 20.0)\; \rm K = 17.9\; \rm K$ .

Let $m$ denote the mass of a sample of specific heat $C$ . Energy required to raise the temperature of this sample by $\Delta T$ :

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

For the neon gas in this question:

$c = 1.03\; \rm J \cdot g^{-1}\cdot K^{-1}$ .
$m = 10.6\; \rm g$ .
$\Delta T = (37.9 - 20.0)\; \rm K = 17.9\; \rm K$ .

Calculate the energy associated with this temperature change:

$\begin{aligned}Q &= c \cdot m \cdot \Delta T \\ &= 1.03\; \rm J \cdot g^{-1}\cdot K^{-1} \times 10.6\; \rm g \times 17.9\; \rm K \\ &\approx 1.95 \times 10^{2}\; \rm J\end{aligned}$ .

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