Use the Heisenberg uncertainty principle to calculate Ax for an electron with AV = 0.170 m/s....

  

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Use the Heisenberg uncertainty principle to calculate Ax for an electron with AV = 0.170 m/s. 1.943x10^-4m ΔΡ = ΜΑV me = 9.10939x10-31 kg h = 6.62608x10-34 Js π = 3.14159265359... By what factor is the uncertainty of the (above) electron's position larger than the diameter of the hydrogen atom? (Assume the diameter of the hydrogen atom is 1.00×10-8 cm.) Use the Heisenberg uncertainty principle to calculate Ax for a ball (mass = 172 g, diameter = 8.30 cm) with Av = 0.170 m/s. The uncertainty of the (above) ball's position is equal to what factor times the diameter of the ball? Use the Heisenberg uncertainty principle to calculate Ax for an electron with AV = 0.170 m/s. 1.943x10^-4m ΔΡ = ΜΑV me = 9.10939x10-31 kg h = 6.62608x10-34 Js π = 3.14159265359... By what factor is the uncertainty of the (above) electron's position larger than the diameter of the hydrogen atom? (Assume the diameter of the hydrogen atom is 1.00×10-8 cm.) Use the Heisenberg uncertainty principle to calculate Ax for a ball (mass = 172 g, diameter = 8.30 cm) with Av = 0.170 m/s. The uncertainty of the (above) ball's position is equal to what factor times the diameter of the ball?

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From uncertainity principle we have AxAph4T Ax h4 Ap given ... View the full answer