How many significant figures are in the measurement 33,050 grams?

Chemistry

1 answer:

aalyn [17]3 years ago

7 0

Answer:

Explanation:

5 digits so 5 sig figures

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The balanced equation for a hypothetical reaction is a + 5b + 6c → 3d + 3e. what is the rate law for this reaction? rate = k [a]

nekit [7.7K]

<u>Answer: </u>The correct rate of the reaction is $Rate=k[a][b]^5[c]^6$

<u>Explanation:</u>

Rate law of the reaction is the expression which expresses the rate of the reaction in the terms of the molar concentrations of the reactants with each term raised to the power of their respective stoichiometric coefficients in a balanced chemical equation.

For the given reaction:

$a+5b+6c\rightarrow 3d+3e$

The expression for the rate law will be: $Rate=k[a][b]^5[c]^6$

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4 years ago

What is hybridization in chemistry? Give some example

dmitriy555 [2]

Answer:

Co2,so2

Explanation:

Hybridization is the mixing of atomic orbitals to form new hybrid orbitals.

Molecule shapes arise from how many hybrid orbitals the central atom uses and how they are arranged.

Don't read the all this but don't forget to leave a ❤

7 0

3 years ago

½O2(g) + H2(g) ⇌ H2O(g)

ira [324]

Answer:

-241.826 kJ·mol⁻¹; -146.9 J·K⁻¹mol⁻¹; 664.6 J·K⁻¹mol⁻¹; spontaneous

Explanation:

½O₂(g) + H₂(g) ⟶ H₂O(g)

ΔHf°/kJ·mol⁻¹: 0 0 -241.826

S°/J·K⁻¹mol⁻¹: 205.0 130.6 188.7

1. ΔᵣH

ΔᵣH = products -reactants = -241.826 -(0 + 0) = -241.826 kJ·mol⁻¹

2. ΔᵣS

ΔᵣS = products - reactants = 188.7 - (205.0 + 130.6) = 188.7 - 335.6 = -146.9 J·K⁻¹mol⁻¹

3. ΔS(univ)

$\begin{array}{rcl}\Delta S_{\text{univ}} &=& \Delta S_{\text{sys}} +\Delta S_{\text{surr}}\\\\ &=& \Delta S_{\text{sys}} -\dfrac{\Delta H_{\text{sys}}}{T}\\\\& = & -146.9 - \dfrac{-241826}{298}\\\\& = & -146.9 + 811.5\\& = & \mathbf{664.6 \,\, J\cdot K^{-1}mol^{-1}}\\\end{array}$

4. Spontaneity

$\begin{array}{rcl}\Delta G &=& \Delta H - T\Delta S\\& = & -241.826 - 298 \times (-0.1469)\\& = & -241.826 + 43.776\\& = & \textbf{-198.050 kJ}\cdot\textbf{mol}^{\mathbf{-1}}\\\end{array}$