How many grams of NaOH are produced from 20 grams of Na2Co3

A sample of the inhalation anesthetic gas Halothane, in a 500-mL cylinder has a pressure of 2.3 atm at 0°C. What will be the pre

STALIN [3.7K]

Answer: 2.56atm

Explanation:

P1/T1=P2/T2

P1T2=P2T1

P2=P1T2/T1

P1=2.3atm

P2=?

T1=0+273=273k

T2=32+273=305k

P2=2.3*305/273

P2=701.5/273

P2=2.56atm

8 0

4 years ago

Read 2 more answers

Hydrogen atoms in a discharge tube are in their ground state. If a beam of free electrons of energy12.9 eV are fired at the hydr

defon

Answer:

See explanation

Explanation:

-0.7ev = -13.6/n^2

n= 4

4--->1

4--->3, 3---> 2, 2--->1

E4-E1= -13.36(1/4^2 - 1/1^2) = 12.53 eV

E4-E3 = -13.36 (1/4^2 - 1/3^2) = 0.65 ev

E3-E2 = -13.36 (1/3^2 - 1/2^2) = 1.86 eV

E2- E1 = -13.6 ( 1/2^2 - 1/1^2) = 10.02 ev

a)

λ= 6.6 × 10^-34 × 3 × 10^8/12.53 × 1.6 × 10^-19

λ= 19.8 × 10^-26/20.048 ×10^-19

λ= 9.9 × 10^ -8 m

b)

λ= 6.6 × 10^-34 × 3 × 10^8/0.65 × 1.6 × 10^-19

λ= 19.8 × 10^-26/1.04 ×10^-19

λ= 19.0 × 10^ -7 m

3 0

3 years ago

Urgent!! will give brainliest!!

Tamiku [17]

An Arrhenius acid is a substance that dissociates in water to form hydrogen ions or protons.

<h3>What is an Arrhenius acid?</h3>

An Arrhenius acid increases the number of $H^+$ ions in the water.

According to the Arrhenius theory, a substance which has hydrogen atom and can easily give hydrogen ion or proton in its aqueous solution is called as Arrhenius acid.

For example, when hydrochloric acid is dissolved in water, it forms chloride ion ( $Cl^-$ ) and hydronium ion ( $H_3O^+$ ).

Learn more about the Arrhenius acid here:

brainly.com/question/9936252

#SPJ1

8 0

2 years ago

One mole of an ideal gas is sealed in a 22.4-L container at a pressure of 1 atm and a temperature of 273 K. The temperature is t

Ket [755]

Answer:

1.11 atm

(P, T)

2.83 atm

0.740 g

0.179 g/L, 0.158 g/L

N₂

Explanation:

One mole of an ideal gas is sealed in a 22.4-L container at a pressure of 1 atm and a temperature of 273 K. The temperature is then increased to 304 K, but the container does not expand. What will the new pressure be?

Assuming ideal behavior, we can calculate the new pressure (P₂) using Gay-Lussac's law.

$\frac{P_{1}}{T_{1}} =\frac{P_{2}}{T_{2}} \\P_{2}=\frac{P_{1}}{T_{1}}.T_{2}=\frac{1atm}{273K} .304K=1.11atm$

The most appropriate formula for solving this problem includes only which variables?

Gay-Lussac's law includes pressure (P) and absolute temperature (T).

Q2) A sample of nitrogen gas in a 1.69-L container exerts a pressure of 1.37 atm at 17 °C. What is the pressure if the volume of the container is maintained constant and the temperature is raised to 327 °C?

Initially the system is at 17°C (290 K) and the temperature is raised to 327°C (600 K). We can calculate the new pressure using Gay-Lussac's law.

$\frac{P_{1}}{T_{1}} =\frac{P_{2}}{T_{2}} \\P_{2}=\frac{P_{1}}{T_{1}}.T_{2}=\frac{1.37atm}{290K} .600K=2.83atm$

Q3) A gas mixture with a total pressure of 770 mmHg contains each of the following gases at the indicated partial pressures: 120 mmHg CO₂, 227mmHg Ar, and 190 mmHg O₂. The mixture also contains helium gas .

What mass of helium gas is present in a 14.0-L sample of this mixture at 282 K?

First, we have to calculate the pressure of Helium. We know that the total pressure is the sum of partial pressures.

Ptotal = pCO₂ + pAr + pO₂ + pHe

pHe = Ptotal - pCO₂ - pAr - pO₂

pHe = 770mmHg - 120mmHg - 227mmHg - 190mmHg=233mmHg

We can calculate the moles of Helium using the ideal gas equation.

$P.V=n.R.T\\n=\frac{P.V}{R.T} =\frac{233mmHg.14.0L}{(0.08206atm.L/mol.K).282K} .\frac{1atm}{760mmHg} =0.185mol$

The molar mass of He is 4.00g/mol.

$0.185mol.\frac{4.00g}{mol} =0.740g$

Calculate the density of oxygen, O₂, under each of the following conditions:

STP

1.00 atm and 35.0 ∘C

Express your answers numerically in grams per liter. Enter the density at STP first and separate your answers by a comma.

STP stands for Standard Temperature and Pressure. The standard temperature is 273 K and the standard pressure is 1 atm.

We can calculate the density using the following expression:

$\rho=\frac{P.M}{R.T} =\frac{1.00atm.4.00g/mol}{(0.08206atm.L/mol.K).273K} =0.179 g/L$

At 1.00 atm and 35.0 °C (308 K)

$\rho=\frac{P.M}{R.T} =\frac{1.00atm.4.00g/mol}{(0.08206atm.L/mol.K).308K} =0.158 g/L$

To identify a diatomic gas (X₂), a researcher carried out the following experiment: She weighed an empty 4.1-L bulb, then filled it with the gas at 2.00 atm and 24.0 ∘C and weighed it again. The difference in mass was 9.5 g . Identify the gas. Express your answer as a chemical formula.

We will look for the molar mass of the compound using the ideal gas equation.

$P.V=n.R.T=\frac{m}{M} .R.T\\M=\frac{m.R.T}{P.V} =\frac{9.5g \times (0.08206atm.L/mol.K)\times 297K }{2.00atm \times 4.1L} =28g/mol$

If the molar mass of X₂ is 28 g/mol, the molar mass of X is 14 g/mol. Then, X is nitrogen and X₂ is N₂.

5 0

3 years ago

please explain why boiling point melting are not considered chemical properties but are considered physical properties of matter

UkoKoshka [18]

Answer:

All matter has physical and chemical properties. Physical properties are characteristics that scientists can measure without changing the composition of the sample under study, such as mass, color, and volume (the amount of space occupied by a sample). Chemical properties describe the characteristic ability of a substance to react to form new substances; they include its flammability and susceptibility to corrosion. All samples of a pure substance have the same chemical and physical properties. For example, pure copper is always a reddish-brown solid (a physical property) and always dissolves in dilute nitric acid to produce a blue solution and a brown gas (a chemical property).

6 0

3 years ago