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masya89 [10]
3 years ago
6

Some hydrogen gas is enclosed within a chamber being held at 200∘C∘C with a volume of 0.0250 m3m3. The chamber is fitted with a

movable piston. Initially, the pressure in the gas is 1.50×106Pa1.50×106Pa (14.8 atmatm). The piston is slowly extracted until the pressure in the gas falls to 0.950×106Pa0.950×106Pa. What is the final volume V2V2V_2 of the container? Assume that no gas escapes and that the temperature remains at 200∘C∘C.
Chemistry
1 answer:
Semenov [28]3 years ago
3 0

Answer:

The final volume is 39.5 L = 0.0395 m³

Explanation:

Step 1: Data given

Initial temperature = 200 °C = 473 K

Volume = 0.0250 m³ = 25 L

Pressure = 1.50 *10^6 Pa

The pressure reduce to 0.950 *10^6 Pa

The temperature stays constant at 200 °C

Step 2: Calculate the volume

P1*V1 = P2*V2

⇒with P1 = the initial pressure = 1.50 * 10^6 Pa

⇒with V1 = the initial volume = 25 L

⇒with P2 = the final pressure = 0.950 * 10^6 Pa

⇒with V2 = the final volume = TO BE DETERMINED

1.50 *10^6 Pa * 25 L = 0.950 *10^6 Pa * V2

V2 = (1.50*10^6 Pa * 25 L) / 0.950 *10^6 Pa)

V2 = 39.5 L = 0.0395 m³

The final volume is 39.5 L = 0.0395 m³

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An electron has _____.
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Answer:

An electron has more mass than a proton or a neutron.

Explanation:

Mass of electron - 9.109 e-31 kg

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7 0
3 years ago
The percent by mass of bicarbonate (HCO3−) in a certain Alka-Seltzer product is 32.5 percent. Calculate the volume of CO2 genera
nevsk [136]

Answer:

The volume of carbon dioxide gas generated 468 mL.

Explanation:

The percent by mass of bicarbonate in a certain Alka-Seltzer = 32.5%

Mass of tablet = 3.45 g

Mass of bicarbonate =3.45 g\times \frac{32.5}{100}=1.121 mol

Moles of bicarbonate ion = \frac{1.121 g/mol}{61 g/mol}=0.01840 mol

HCO_3^{-}(aq)+HCl(aq)\rightarrow H_2O(l)+CO_2(g)+Cl^-(aq)

According to reaction, 1 mole of bicarbonate ion gives with 1 mole of carbon dioxide gas , then 0.01840 mole of bicarbonate ion will give:

\frac{1}{1}\times 0.01840 mol=0.01840 mol of carbon dioxide gas

Moles of carbon dioxide gas  n = 0.01840 mol

Pressure of the carbon dioxide gas = P = 1.00 atm

Temperature of the carbon dioxide gas = T = 37°C = 37+273 K=310 K

Volume of the carbon dioxide gas = V

PV=nRT (ideal gas equation)

V=\frac{nRT}{P}=\frac{0.01840 mol\times 0.0821 atm L/mol K\times 310 K}{1.00 atm}=0.468 L

1 L = 1000 mL

0.468 L =0.468 × 1000 mL = 468 mL

The volume of carbon dioxide gas generated 468 mL.

5 0
3 years ago
given the following reaction: CuO (s) + H2 (g) to Cu(s) + H2O (g). If 250 L of hydrogen gas are used to reduce copper (II) oxide
QveST [7]

24g is needed no explanation

4 0
3 years ago
Write the symbol for each of the following ions:
kap26 [50]

Answer:

a) _{31}^{71}\textrm {P^{3+}}

b) _{35}^{80}\textrm {Br^{-}}

c) _{90}^{232}\textrm {Th^{4+}}

d) _{38}^{87}\textrm {Sr^{2+}}

Explanation:

For neutral atoms:

Atomic Number (Z)= number of protons = number of electrons

Mass number (A) = number of protons + number of neutrons

For ions with positive net charge:

Number of protons = Z + net charge

For ions with negative net charge:

Number of protons= Z - net charge

a) A = 71, Charge = +3

Number of electrons = 28

Number of protons = 28 +3 =31

_{31}^{71}\textrm {P^{3+}}

b)  A = 35, Z = 45+35=80, Charge = -1

Number of protons =35

Number of neutrons = 45

Number of electrons = 36

Charge = Number of protons- Number of electrons =35-36 = -1

_{35}^{80}\textrm {Br^{-}}

c)  Charge = +4

Number of electrons = 86

Number of protons = Z = 86+4 = 90

mass number = A = 90+142 = 232

_{90}^{232}\textrm {Th^{4+}}

d)  Charge = +2

Atomic number = Number of protons = Z = 38

mass number = A = 87

_{38}^{87}\textrm {Sr^{2+}}

3 0
3 years ago
The first order reaction of methyl isonitrile to form acetonitrile has a rate constant of k = 1.7 × 10−15 at 298 K. What will ha
ludmilkaskok [199]
Refer to to this chart 

Credits to <span>https://image.slidesharecdn.com/nybf09-unit2slides26-57-100125181507-phpapp01/95/nyb-f09-unit-2-slid...

As temperature decreases, rate decreases. 

As temp increases, k also increases. </span>

3 0
3 years ago
Read 2 more answers
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