Does a hypothesis have to be true for a experiment to be valid?

Step2247 [10]

<h2>Hello!</h2>

The answer is:

Hence, the new pressure will be 2.07 atm.

$P_{2}=2.07atm$

Since we know that the gas is inside of a rigid container, meaning that the volume will be kept constant, we can solve the problem using the Gay-Lussac's Law.

The the Gay-Lussac's Law establishes that when an ideal gas is kept at the same volume, the pressure and the temperature will be proportional.

We need to pay special attention when we are working with the Gay-Lussac's Law since its equaitons works with absolute temperatures (Kelvin ), so, if we are working with relative temperatures such as Celsius degrees or Fahrenheit degrees, we need to convert the temperatures to Kelvin.

We can convert from Celsius degrees to Kelvin using the following formula:

$Temperature(K)=Temperature(C\°)+273$

So, we have the Gay-Lussac's equation:

$\frac{P_{1}}{T_{1}}=\frac{P_{2}}{T_{2}}$

Also, we are given the following information:

$T_{1}=30\° \\P_{1}=2atm\\T_{2}=40\°$

Therefore, converting the temperature to Kelvin, we have:

$T_{1}=30C\°=30+273K=303K\\\\T_{1}=40C\°=40+273K=313K\\$

Now, calculating we have:

$\frac{P_{1}}{T_{1}}=\frac{P_{2}}{T_{2}}$

$P_{2}=\frac{P_{1}}{T_{1}}*T_{2}\\\\P_{2}=\frac{2atm}{303K}*313K=2.07atm$

Hence, the new pressure will be 2.07 atm.

$P_{2}=2.07atm$

Have a nice day!

4 0

4 years ago

Use the fact that to determine how much the pressure must change in order to lower the boiling point of water by a small amount

erma4kov [3.2K]

Complete Question

Use the fact that $d\mu=\frac{V}{N}dp-\frac{s}{N}dT$ to determine how much the pressure must change in order to lower the boiling point of water by a small amount 3.20e-01 K. You may assume that the entropy and density of the liquid and gas are roughly constant for these small changes. You may also assume that the volume per molecule of liquid water is approximately zero compared to that of water vapor, and that water vapor is an ideal gas. Useful constants: Atmospheric pressure is 101300 Pa The boiling point of water at atmospheric pressure is 373.15 K The entropy difference between liquid and gas per kilogram is 6.05e 03 J/kgK The molecular weight of water is 0.018 kg/mol. (a) 0.00e 00 Pa (b) 1.14e 03 Pa (c) 6.85e 26 Pa (d) 4.24e 05 Pa (e) 3.81e 28 Pa

Answer:

Correct option is B

Explanation:

From the question we are told that:

Given Equation $d\mu=\frac{V}{N}dp-\frac{s}{N}dT$

Change of boiling point \triangle $H=3.20e-01 K$

Generally the equation for Change in time is mathematically given by

$d\mu=\frac{V}{N}dp-\frac{s}{N}dT$

$dp=\frac{s}{v}dT$

Where

$s=Entropy\ difference *molar\ weight$

$s=6.05*10^3*0.018j/mol.k$

And

$V=\frac{RT}{P}$ (from ideal gas equation)

Therefore

$dp=\frac{Ps}{RT}dT$

$dp=\frac{101300*6.05*10^3*0.018}{8.314*373.15}3.20*10^{-1}$

$dp=1137.873pa$

$dp=1.14e 03 Pa$

Therefore correct option is B

4 0

3 years ago

Transfer 2-3 drops of each solution onto the indicator paper. Be sure to

alexira [117]

Answer:

0.1 M HCl pH: 1-2

0.001 M HCl pH: 3-4

0.00001 M HCl pH: 5-6

Distilled Water pH: 7

0.00001 M NaOH pH: 8-9

0.001 M NaOH pH: 10-11

0.1 M NaOH pH: 12-13

Explanation:

4 0

3 years ago

Sodium hydroxide, NaOH; sodium phosphate, Na3PO4; and sodium nitrate, NaNO3, are all common chemicals used in cleanser formulati

Sholpan [36]

Start by writing out molar mass of each component:

1) NaOH= 22.99+16+1.01 --> 40

2) Na₃PO₄= (22.99)3 + 94.97 + 64 --> 227.94

3) NaNO₃= 22.99 + 14 + 48 --> 84.99

Now compare the mass of sodium with the rest of the substances:

1) (22.99/40)100%= 57.475%

2) (68.97/227.94)/100%= 30.25%

3) (22.99/84.99)/100%= 27.05%

As seen, the ordered list is: Sodium hydroxide, sodium phosphate and sodium nitrate.

Hope I helped :)

8 0

4 years ago

Match the vocabulary word with its definition. Match the items in the left column to the items in the right column. 1. The actua

tekilochka [14]

Answer:

1. The actual amount of product that is produced from a given amount of reactant or reactants. → actual yield

2. A law which states that in ordinary chemical reactions, the sum of the masses of the reactants always equals the sum of the masses of the products. → Conservation of Mass

3. The reactant that is not used up in a reaction that goes to completion

→ excess reactant

4. The reactant that limits how much product is produced in a reaction that goes to completion. It is used up in the reaction. → limiting reactant

5. The ratio of the actual yield to theoretical yield multiplied times 100.

→ percent yield

6. The maximum calculated amount of product produced from a given reactant in a reaction that goes to completion. → theoretical yield

7. The study of the quantitative relationships between reactants and products in a chemical reaction. → stoichiometry

Explanation:

1. The actual amount of product that is produced from a given amount of reactant or reactants. → actual yield

The actual yield is the actual amount of product that is produced in a chemical reaction and it can be determined experimentally.

2. A law which states that in ordinary chemical reactions, the sum of the masses of the reactants always equals the sum of the masses of the products. → Conservation of Mass

The law of conservation of mass states that mass in an isolated closed system is neither created nor destroyed by chemical reactions or physical transformations. According to the law of conservation of mass, the mass of the products in a chemical reaction must equal the mass of the reactants.

3. The reactant that is not used up in a reaction that goes to completion

→ excess reactant

In any chemical reaction between two or more reactants, the excess reactant is the substance that is leftover when the chemical reaction is ended. The amount of product formed is not limited by this reagent.

4. The reactant that limits how much product is produced in a reaction that goes to completion. It is used up in the reaction. → limiting reactant

In any chemical reaction between two or more reactants, the limiting reactant is the substance that is consumed completely when the chemical reaction is ended. The amount of product formed is limited by this reagent, since the reaction cannot continue without it.

5. The ratio of the actual yield to theoretical yield multiplied times 100.

→ percent yield

percent yield = (actual yield / theoretical yield) *100

6. The maximum calculated amount of product produced from a given

reactant in a reaction that goes to completion.

→ theoretical yield

theoretical yield is defined as the amount of the obtained desired product.

7. The study of the quantitative relationships between reactants and products in a chemical reaction.

→ Stoichiometry

Stoichiometry is a branch of chemistry that deals with relationships between reactants and/or products in a reaction to determine desired quantitative data.

3 0

3 years ago