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What is the chemical formula for the ionic compound formed by Au3+ and
HSO3-?

Answers

Answer 1

Answer:

Answer:

The chemical formula for the ionic compound formed by Au3+ and

HSO3-compound is Au(HSO3)3

Explanation:

The charge on Au ion is $+3$

And the charge on HSO3- is $-1$

Thus, the number of atoms required by HSO3- to complete its octate is 1. On the other hand Au has 3 excess ions and hence it is to be released to reach the stable state.

So three molecules of HSO3- will combine with one atom of Au 3+

Thus, the compound formed by these two is Au(HSO3)3

Answer 2

Answer:

Final answer:

The chemical formula for the ionic compound formed by Au3+ and HSO3- is Au(HSO3)3, as ionic compounds are always neutral.

Explanation:

The ionic compound formed by Au3+ (Gold ion) and HSO3- (Bisulfite ion) must have a net charge of zero since ionic compounds are neutral. Hence, we need 3 bisulfite ions to balance out one gold ion, which gives us the chemical formula as Au(HSO3)3.

Indeed, the formation of ionic compounds is a fascinating process. It involves the transfer of electrons from one atom (usually a metal) to another (usually a nonmetal), resulting in the formation of ions. These ions are then attracted to each other due to their opposite charges, forming an ionic compound. In this case, the gold ion (Au3+) donates three electrons, which are accepted by three bisulfite ions (HSO3-). This results in a neutral compound, as the positive and negative charges balance each other out. The resulting compound, Au(HSO3)3, is an example of how elements can combine in specific ratios to form neutral compounds.

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1. Potassium (K) has an atomic mass of 39.0983 amu and only two naturally-occurring isotopes. The K-41 isotope (40.9618 amu) has a natural abundance of 6.7302%. What is the mass (in amu) of the other isotope

What is the purpose of a catalyst?O A. To change the potential energy of the reactants
O B. To lower the activation energy of a reaction
O C. To increase the kinetic energy of the reactants
O D. To shift the equilibrium position of a reaction

Answers

B. To lower the activation energy of a reaction

Answer:

To lower the activation energy of a reaction

Explanation:

i just took the test and got it right ...... i hope this helps :)

Calculate the enthalpy for this reaction: 2C(s) + H2(g) ---> C2H2(g) ΔH° = ??? kJ Given the following thermochemical equations: C2H2(g) + (5/2)O2(g) ---> 2CO2(g) + H2O(ℓ) ΔH° = -1,123 kJ C(s) + O2(g) ---> CO2(g) ΔH° = -340 kJ H2(g) + (1/2)O2(g) ---> H2O(ℓ) ΔH° = -211 kJ

Answers

Answer:

The enthalpy for given reaction is 232 kilo Joules.

Explanation:

$C_2H_2(g) + (5)/(2)O_2(g)\rightarrow 2CO_2(g) + H_2O(l), \Delta H^o_(1) = -1,123 kJ$ ...[1]

$C(s) + O_2(g)\rightarrow CO2(g), \Delta H^o_(2) = -340 kJ$ ..[2]

$H_2(g) + (1)/(2)O_2(g)\rightarrow H_2O(l) ,\Delta H^o_(3) = -211 kJ$ ..[3]

$2C(s) + H_2(g)\rightarrow C_2H_2(g),\Delta H^o_(4) =?$ ..[4]

2 × [2] + [3] - [1] ( Using Hess's law)

$\Delta H^o_(4)=2* \Delta H^o_(2)+\Delta H^o_(3) - \Delta H^o_(1)$

$\Delta H^o_(4)=2* (-340 kJ) + (-211 kJ) - (-1,123 kJ)$

$\Delta H^o_(4)=232 kJ$

The enthalpy for given reaction is 232 kilo Joules.

Scaled Synthesis of Alum. Show your calculations for:a.the experimental scaling factor giving rise to a 15.0 g theoretical yield;b.the corrected volumes of KOH and H2SO4; andc.the theoretical yield of alum based on the actual amount of Al used.Make sure you carefully show each step for these calculations.

Answers

Answer:

Explanation:

You don't give your experimental data, so I shall assume:

Mass of Al = 1.07 g

20 mL of 3 mol·L⁻¹ KOH

20 mL of 9 mol·L⁻¹ H₂SO₄

The overall equation for the reaction is

Mᵣ: 26.98 474.39

2Al + 2KOH +4H₂SO₄ + 22H₂O ⟶ 2K[Al(SO₄)₂]·12H₂O + 3H₂

m/g: 1.07

(c) Theoretical yield of alum

(i) Moles of Al

$\text{Moles of Al} = \text{1.07 g Al} * \frac{\text{1 mol Al}}{\text{26.98 g Al}} = \text{0.039 66 mol Al}$

(ii) Moles of alum

$\text{Moles of alum} = \text{0.039 66 mol Al} * \frac{\text{2 mol alum }}{\text{2 mol Al}} = \text{0.039 66 mol alum \n}$

(iii) Theoretical yield of alum

$\text{Mass of alum} = \text{0.039 66 mol alum} * \frac{\text{474.39 g alum}}{\text{1 mol alum}} = \textbf{18.8 g alum}$

(a) Scaling factor for 15.0 g alum

You want a theoretical yield of 15.0 g, so you must scale down the reaction.

$\text{Scale factor} = (15.0)/(18.8) = \mathbf{0.798}$

(b) Corrected volumes of NaOH and H₂SO₄

V = 0.798 × 20 mL = 16 mL

A student is heating a chemical in a beaker with a Bunsen burner.In a paragraph of at least 150 words, identify the safety equipment that should be used and the purpose of it for the given scenario.

Answers

When a student is warming a chemical in a container using a special burner, it is very important to focus on safety by using the right safety tools.

What is the safety equipment

First, the student needs to wear the right safety clothes like a lab coat, gloves, and goggles to protect themselves from getting splashed or hurt by chemicals. A lab coat stops chemicals from touching the skin, gloves keep the hands safe, and safety goggles protect the eyes from chemicals

and hot things.

Furthermore, using a fume hood is necessary to make sure there is enough fresh air circulating and to remove any dangerous fumes or gases that might be released while heating things up.

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Answer:The student should be wearing a lab coat or maybe an apron to prevent chemicals from spilling or exploding onto their clothes, I do recommend a lab coat better though because it can protect your skin better. Next, make sure while messing with chemicals you are always wearing goggles, if you are not wearing them there is a chance that after touching chemicals you could touch your eyes. And that brings me to washing your hands straight away after messing with chemicals. You could also wear gloves and just take them off when you're done but if you don't have clean hands afterward you could always put the chemicals all over your skin. But in case you do touch your eyes there is always an emergency eyewash station somewhere in the lab room. And if you are to get Chemicals on your skin, in your hair, on your clothes, or to be on fire, there shall be a shower somewhere to get rid of that. But if you read the instructions or listen closely to the teacher you shall have no problem.

Explanation:

I kinda got off topic

Using the balanced equation below,how many grams of carbon dioxide
would be produced from the
complete reaction of 83.7 g carbon
monoxide?
Fe2O3 + 3CO → 2Fe + 3CO2

Answers

131.6 grams of carbon dioxide would be produced from the complete reaction of 83.7 g carbon monoxide.

The balanced chemical equation is given below.

Fe2O3 + 3CO → 2Fe + 3CO2

Calculation,

Since, 28g of carbon dioxide produces 44g of carbon monoxide.

So, 83.7 g of carbon dioxide produces 44×83.7/28 grams

83.7 g of carbon dioxide produces 131.6 grams

What is chemical equation?

The symbolic representation of chemical reaction in which reactant represents in left side and product represents in right side is called chemical equation.

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Answer:131.6 g

Explanation:

How many grams of NaBr must he measure out to have 4.20 moles?