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3 years ago

Which substance is a base? HCOOH RbOH H2CO3 NaNO3

Chemistry

2 answers:

harkovskaia [24]3 years ago

7 0

Answer:

RbOH

Explanation:

Alex Ar [27]3 years ago

6 0

Answer:

RbOH

Explanation:

For this question, we have to remember what is the definition of a base. A base is a compound that has the ability to produce hydroxyl ions $OH^-$ , so:

$AOH~->~A^+~+~OH^-$

With this in mind we can write the reaction for each substance:

$HCOOH~->~HCOO^-~+~H^+$

$RbOH~->~Rb^+~+~OH^-$

$H_2CO_3~->~CO_3^-^2~+~2H^+$

$NaNO_3~->~Na^+~+~NO_3^-$

The only compound that fits with the definition is $RbOH$ , so this is our base.

I hope it helps!

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How many electrons can be contained in the second energy level?

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Its D for the second energy level, but the first energy level is 2.

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Nitric acid decomposes in light to form nitrogen dioxide, water, and oxygen, according to the following chemical equation.

geniusboy [140]

Answer:

b. 0.22 L

Explanation:

Step 1: Write the balanced equation

4 HNO₃(l) ⇒ 4 NO₂(g) + 2 H₂O(l) + O₂(g)

Step 2: Calculate the moles corresponding to 2.5 g of HNO₃

The molar mass of HNO₃ is 63.01 g/mol.

2.5 g × 1 mol/63.01 g = 0.040 mol

Step 3: Calculate the moles of O₂ produced from 0.040 moles of HNO₃

The molar ratio of HNO₃ to O₂ is 4:1. The moles of O₂ produced are 1/4 × 0.040 mol = 0.010 mol.

Step 4: Calculate the volume corresponding to 0.010 moles of O₂

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7 0

3 years ago

Student 1You are supplied with a 100 mL beaker that you weigh on a pocket balance – its weight clean and dry is 29.3 g. You then

navik [9.2K]

Answer:

The answer to your question is: density = 0.993 g/ml

Explanation:

Data

mass beaker empty = 29.3 g

volume of liquid = 15 ml

mass beaker + liquid = 44.2 g

Formula

density = mass / volume

Process

mass of liquid = 44.2 - 29.3

= 14.9 g

density = 14.9 / 15

= 0.993 g/ml

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3 years ago

The compound consists of 40% carbon and 6.71% hydrogen. Its mass of 1 liter of steam is 2.4 g. What is the formula of the compou

AveGali [126]

I think it is CH2O.

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3 years ago

Calculate the equilibrium constant for the reaction: 2 Cr + 3 Pb2+ ----> 3 Pb + 2 Cr3+ at 25oC. Eocell = 0.61 V

sattari [20]

Answer:

The value is $K = 8*10^{61}$

Explanation:

From the question we are told that

The equation is $2 Cr + 3Pb^{2+} \to 3Pb + 2Cr^{3+}$

The temperature is $T = 25^oC = 298 K [room \ temperature ]$

The emf at standard condition is $E^o_{cell} = 0.61 \ V$

Generally at the cathode

$3Pb^{2+}(aq) + 6 e- --> 3Pb(s)$

At the anode

$2Cr^{3+} + 6e^- \to 2Cr$

Generally for an electrochemical reaction, at room temperature the Gibbs free energy is mathematically represented as

$G = n* F * E^o_{cell}$

Here n is the no of electron with value n = 6

F is the Faraday's constant with value 96487 J/V

=> $G = 6 * 96487 * 0.61$

=> $G = 3.5 *10^{5} \ J$

This Gibbs free energy can also be represented mathematically as

$G = RTlogK$

Here R is the cell constant with value 8.314J/K

K is the equilibrium constant

From above

=> $K = antilog^{\frac{G}{ RT} }$

Generally antilog = 2.718

=> $K = 2.718^{\frac{3.5 *10^5}{ 8.314* 298} }$

=> $K = 8*10^{61}$

6 0

3 years ago