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MrRissso [65]
3 years ago
5

Consider an electron with a mass of 9.11 x 1051 kg and a 100.0 g tennis ball that are both moving with a velocity of 70.0 m s1.

(a) Calculate the momentum of the electron (p mv). (b) Calculate the momentum of the tennis ball (c) What is the uncertainty in the position of the electron (Ax) if the uncertainty in its momentum (Ap) is equal to 1.0 % of p for the electron? (d) What is the uncertainty in the position of the tennis ball (Ax) if the uncertainty in momentum (Ap) is equal to 0.1% of p for the tennis ball? (e) Comment on how the uncertainty in position (Ax) compares to the overall size in each case
Chemistry
1 answer:
MrRissso [65]3 years ago
5 0

Answer:

(a) 6.38 × 10⁻²⁹ kg·m·s⁻¹; (b) 7.00 kg·m·s⁻¹; (c) 82.7 µm; (d) 7.53 × 10⁻³⁴  m;

(e) Δx ∝ 1/m

Explanation:

(a) Momentum of electron

p = mv = 9.11  × 10⁻³¹ kg × 70.0 m·s⁻¹ = 6.38 × 10⁻²⁹ kg·m·s⁻¹

(b) Momentum of tennis ball

p = mv = 0.1000 kg × 70.0 m·s⁻¹ = 7.00 kg·m·s⁻¹

(c) Δx for electron

Δp = 0.010p = 0.010 × 6.38 × 10⁻²⁹ kg·m·s⁻¹ = 6.38 × 10⁻³¹ kg·m·s⁻¹

\begin{array}{rcl}\Delta x \Delta p & \geq & \dfrac{h}{4 \pi}\\\\\Delta x \times 6.38 \times 10^{-31} \text{ kg$\cdot$m$\cdot$s$^{-1}$} & \geq & \dfrac{6.626 \times 10^{-34} \text{ kg$\cdot$m$^{2}$s}^{-1}}{4 \pi}\\\\\Delta x \times 6.38 \times 10^{-31} & \geq & 5.273 \times 10^{-35} \text{ m}\\\Delta x & \geq & \dfrac{5.273 \times 10^{-35} \text{ m}}{6.38 \times 10^{-31}}\\\\ & \geq&8.27 \times10^{-5} \text{ m}\\ &\geq&\textbf{82.7 $\mu$m}\\\end{array}

(d) Δx for tennis ball

Δp = 0.010p = 0.010 × 7.00 kg·m·s⁻¹ = 0.0700 kg·m·s⁻¹

\begin{array}{rcl}\Delta x \times 0.0700 & \geq & 5.273 \times 10^{-35} \text{ m}\\\Delta x & \geq & \dfrac{5.273 \times 10^{-35} \text{ m}}{0.0700}\\\\ &\geq& \textbf{7.53 $\mathbf{\times 10^{-34}}$ m}\\\end{array}

(e) Relative uncertainty

Both particles are travelling at the same speed, so,

ΔxΔp = Δx × mv = mvΔx = constant

v is constant, so  

Δx ∝ 1/m

Thus, the larger the mass of an object, the smaller the uncertainty in its velocity.

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I2(g) + Cl2(g)2ICl(g) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 1.62 mol
galina1969 [7]

Answer:

The change in entropy of the surrounding is -146.11 J/K.

Explanation:

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Enthalpy of formation of chlorine gas = \Delta H_f_{(Cl_2)}=0 kJ/mol

Enthalpy of formation of ICl gas = \Delta H_f_{(ICl)}=17.78 kJ/mol

The equation used to calculate enthalpy change is of a reaction is:  

\Delta H_{rxn}=\sum [n\times \Delta H_f(product)]-\sum [n\times \Delta H_f(reactant)]

For the given chemical reaction:

I_2(g)+Cl_2(g)\rightarrow 2ICl(g),\Delta H_{rxn}=?

The equation for the enthalpy change of the above reaction is:

\Delta H_{rxn}=[(2\times \Delta H_f_{(ICl)})]-[(1\times \Delta H_f_{(I_2)})+(1\times \Delta H_f_{(Cl_2)})]

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Enthaply change when 1.62 moles of iodine gas recast:

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Entropy of the surrounding = \Delta S^o_{surr}=\frac{\Delta H}{T}

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1 kJ = 1000 J

The change in entropy of the surrounding is -146.11 J/K.

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