Un gas ocupa un volumen de 358L a 152°C y 470 mmHg ¿Qué volumen ocupara el gas, si la temperatura aumente a 500 K y 6 atm?
1 answer:
Answer:
42 L
Explanation:
de los parámetros en la pregunta;
V1 = 358L
T1 = 152 ° C + 273 = 425 K
P1 = 470 mmHg × 1 atm / 760 mmHg = 0.6atm
V2 =?
P2 = 6 atmósferas
T2 = 500 K
P1V1 / T1 = P2V2 / T2
P1V1T2 = P2V2T1
V2 = P1V1T2 / P2T1
V2 = 0,6 × 358 × 500/6 × 425
V2 = 107400/2550
V2 = 42 L
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<em>Answer:</em>
- The option C is correct.
- CH4N, 90g, C3H12N3.
<em>Explanation:</em>
<em>Option C:</em>
- The molecular formula is C3H12N3.
- If we take ratio 3:12:3 that will be equal to 1:4:1 so its empirical formula will be CH4N.
- The molar mass of molecular formula = (12×3) + (1×12) +( 14×3) = 98 g
<em>Option A :</em>
- In option A , molecular and empirical formula are both correct but molar mass is not valid. It should be 169 acc. to molecular formula.
<em>Option B:</em>
- In option B, molecular formual is not valid.
- It should be as C6H16O2
